Solute in a sentence

(1) The solvent delocalizes the solute.

(2) The solute easily dissolves in dioxide.

(3) The solute slowly dissolves in dioxide.

(4) The antipoles of a solvent are the solute.

(5) The solvent will dissolve through the solute.

(6) The solute was redissolved in a polar solvent.

(7) The solute dissolved completely in the solvent.

(8) The water-bath was used to dissolve the solute.

(9) The solution was undersaturated with the solute.

(10) Adding more solvent helps the solute redissolve.

Solute sentence

(11) The solute dissolved slowly in the cold solution.

(12) The miscible solvents quickly dissolve the solute.

(13) The solute was redissolved by adding a surfactant.

(14) The solute particles dispersed evenly in solution.

(15) The solute dissolved readily in the acidic solution.

(16) The solute was redissolved by filtering the mixture.

(17) The solute redissolves as the temperature increases.

(18) The solute recrystallises as the solvent evaporates.

(19) The solute was redissolved by increasing the pressure.

(20) The supernate was evaporated to concentrate the solute.

Solute make sentence

(21) The osmotically active solute in this solution is urea.

(22) The solute dissolved faster when the solution was heated.

(23) Solvate molecules can interact with other solute species.

(24) The solvated ions interacted with other solute molecules.

(25) The solute recrystallises out of the solvent as it cools.

(26) The solute concentration was expressed in moles per liter.

(27) The solute dissolved slowly in the presence of a catalyst.

(28) The osmotically active solute in this solution is glucose.

(29) The solute particles redissolve as the pressure decreases.

(30) The desolvation of a solute can be achieved by filtration.

Sentence of solute

(31) The neutral solution was used as a solvent for the solute.

(32) Adding more solute to the solution increased its viscosity.

(33) The miscible solvents enhance the solubility of the solute.

(34) The solute molecules adsorb onto the chromatography column.

(35) The osmotically active solute in this solution is mannitol.

(36) Please explain the difference between a solute and solvent.

(37) The solute concentration was measured using a refractometer.

(38) The solute redissolves as the pH level becomes more neutral.

(39) The solute molecules recrystallise into a lattice structure.

(40) The concentration of the solute equilibrated in the solvent.

Solute meaningful sentence

(41) The apolar solvent was used to dissolve the nonpolar solute.

(42) The solute redissolves as the solution is stirred vigorously.

(43) The solvation of a solute can affect its chemical reactivity.

(44) Solvation is the process of dissolving a solute in a solvent.

(45) The solvent will dissolve through the solute in the solution.

(46) Dilute after taking into account the solubility of the solute.

(47) The dissolved solute recrystallizes as the solvent evaporates.

(48) The solute dissolved completely, resulting in a clear solution.

(49) Pour into the beaker and stir it gently to dissolve the solute.

(50) The miscible solvents ensure complete dissolution of the solute.

Solute sentence examples

(51) The solution was left undisturbed to allow the solute to settle.

(52) The solute recrystallises into a pure form as the solvent cools.

(53) The molality of the solution increased as more solute was added.

(54) The molarity of the solution was increased by adding more solute.

(55) The solute concentration was determined using a titration method.

(56) The solute concentration was higher in the concentrated solution.

(57) The solute recrystallises into a solid upon cooling the solution.

(58) The absorbance of the solution increased as more solute was added.

(59) The solute particles were too small to be seen with the naked eye.

(60) Osmolarity is a measure of the solute concentration in a solution.

Sentence with solute

(61) The chemist heated the solution to bring up to density the solute.

(62) The solute dissolved slowly in solution due to its low solubility.

(63) The desolvation of a solute can be enhanced by using a desiccator.

(64) When the solution was cooled, the solute began to precipitate out.

(65) The chemical action of the solvent dissolved the solute completely.

(66) The solute particles in an aqueous solution are evenly distributed.

(67) The undersaturated solution was unable to dissolve any more solute.

(68) The solid will precipitate under the right concentration of solute.

(69) The solvation of a solute can be enhanced by stirring the solution.

(70) The solution remained undersaturated even after adding more solute.

Use solute in a sentence

(71) The solution was heated to encourage the solute to precipitate out.

(72) The desolvation of a solute can result in the formation of crystals.

(73) The solute particles were evenly distributed throughout the solvent.

(74) The solute concentration affected the rate of the chemical reaction.

(75) The color of an aqueous solution can change depending on the solute.

(76) The desolvation of a solute can result in changes in its solubility.

(77) The absorptivity of the solution increased, so we added more solute.

(78) The supersaturated solution was heated to dissolve the excess solute.

(79) The solute concentration affected the freezing point of the solution.

(80) The slow evaporation of the solvent caused the solute to crystallize.

Sentence using solute

(81) The solute redissolves as the concentration of the solvent increases.

(82) The solute particles formed a precipitate when added to the solution.

(83) The solute particles were evenly distributed throughout the solution.

(84) The solute particles settled at the bottom of the solution over time.

(85) The solute dissolved readily in solution, indicating high solubility.

(86) The desolvation of a solute can be achieved by adding a drying agent.

(87) The mols of a solute can be calculated using its mass and molar mass.

(88) The desolvation of a solute can be affected by the pH of the solution.

(89) The solute molecules formed hydrogen bonds with the solvent molecules.

(90) The solvated substance exhibited enhanced solute-solvent interactions.

Solute example sentence

(91) The molal concentration of the solute was expressed in units of molal.

(92) The osmolality of a solution is a measure of its solute concentration.

(93) The solution is left to evaporate, allowing the solute to crystallise.

(94) The desolvation of a solute can be accelerated by using a vacuum pump.

(95) The critical temperature of a liquid can be lowered by adding a solute.

(96) The solute concentration affected the osmotic pressure of the solution.

(97) The solute particles were attracted to the charged ions in the solvent.

(98) The concentration of a solute in an aqueous solution can be calculated.

(99) The desolvation of a solute can be accelerated by using a drying agent.

(100) The solvation of a solute can result in the formation of hydrated ions.

Sentence with word solute

(101) The solvation of a solute can affect its solubility in a given solvent.

(102) The optical density of the solution increased as more solute was added.

(103) The diffusivity of a solute in a solvent affects the rate of diffusion.

(104) Osmotic pressure is affected by the size and charge of solute particles.

(105) Osmolality is a measure of the total solute concentration in a solution.

(106) The solute particles dispersed unevenly in the solution, forming clumps.

(107) The solute particles moved freely in solution due to their random motion.

(108) The choice of precipitants can be influenced by the nature of the solute.

(109) The specific volume of a solution depends on the concentration of solute.

(110) The molal concentration of the solute was measured using a refractometer.

Sentence of solute

(111) The desolvation of a solute can result in the formation of a precipitate.

(112) The vapour-pressure of a solution depends on the concentration of solute.

(113) Increasing the concentration of the solute resulted in a higher molarity.

(114) The solvation of a solute can lead to changes in its physical properties.

(115) The liquidus temperature of a solution can be lowered by adding a solute.

(116) The liquid solution was agitated gently to dissolve the solute completely.

(117) The desolvation of a solute can be accelerated by applying heat or vacuum.

(118) The desolvation of a solute can be hindered by the presence of impurities.

(119) The strength of solvation depends on the nature of the solute and solvent.

(120) Adding more solute to a solution will increase its colligative properties.

Solute used in a sentence

(121) The solute concentration was inversely proportional to the solvent volume.

(122) The solute was added gradually to the solvent to dissolve nitrogen slowly.

(123) The diffusional rate of a solute depends on its molecular weight and size.

(124) The molal concentration of the solute was lower than the initial estimate.

(125) The molal concentration of the solute was adjusted by adding more solvent.

(126) The desolvation of a solute can be influenced by temperature and pressure.

(127) The solvation of a solute can lead to the formation of solvated complexes.

(128) Solvation is influenced by the nature of the solute and solvent molecules.

(129) The solution reached a state of super-saturation due to the excess solute.

(130) The concentration of the solute was uniform isotropically in the solution.

Solute sentence in English

(131) Increasing the temperature of the solution increased the solute solubility.

(132) The solute particles moved randomly in the solution due to Brownian motion.

(133) The molal concentration of the solution increased as more solute was added.

(134) The molal concentration of the solute was found to be higher than expected.

(135) The desolvation of a solute can lead to changes in its chemical reactivity.

(136) The desolvation of a solute can result in the formation of a solid residue.

(137) The solvation of a solute can result in changes in its physical properties.

(138) The solvation of a solute can be quantified using thermodynamic parameters.

(139) The mixture is left to cool slowly, allowing the solute to crystallise out.

(140) The desolvation of a solute can lead to changes in its physical properties.

(141) The maximum density of the solution was achieved by adding a denser solute.

(142) The solvation of a solute can be affected by the presence of other solutes.

(143) The solvation of a solute can result in changes in its chemical reactivity.

(144) The concentration of the solute equilibrated in the solvent after stirring.

(145) The supersaturated solution was slowly evaporated to concentrate the solute.

(146) Molality is a useful unit for expressing the amount of solute in a solution.

(147) The dissolvent was carefully chosen to ensure compatibility with the solute.

(148) The concentration of a solute in an aqueous solution affects its properties.

(149) The molal concentration of the solute was directly proportional to pressure.

(150) The solute concentration in solution was measured using a spectrophotometer.

(151) The solvation of a solute can affect its solubility in a particular solvent.

(152) The solution is left to stand overnight, allowing the solute to crystallise.

(153) The solvation of a solute can result in the formation of solvated complexes.

(154) The diffusibility of a solute in a solvent determines the rate of diffusion.

(155) The fugacity of the solute in the solution was calculated using Henry's law.

(156) The desolvation of a solute can be influenced by the polarity of the solvent.

(157) The solute dissolved spontaneously in the solvent without any external force.

(158) The solute particles formed a precipitate when mixed with a specific reagent.

(159) The osmolarity of a solution refers to its concentration of solute particles.

(160) The desolvation of a solute can be hindered by the presence of other solutes.

(161) The apolar solvent was used to dissolve the nonpolar solute for the reaction.

(162) The miscible nature of the solvents allows for easy dissolution of the solute.

(163) The molal concentration of the solute in the solution decreased with dilution.

(164) The percentage composition of a solution can be altered by adding more solute.

(165) The solvation of a nonpolar solute in a polar solvent is often less favorable.

(166) The solute recrystallises into individual crystals as the solution cools down.

(167) The solute particles diffused through the solution due to their kinetic energy.

(168) The solute particles were too large to pass through the semipermeable membrane.

(169) The solute particles were attracted to the polar ends of the solvent molecules.

(170) The manometrically determined concentration of the solute was 1 mole per liter.

(171) The molality of a solution can be used to determine the solubility of a solute.

(172) The molality of a solution can be used to calculate the molar mass of a solute.

(173) The miscible nature of the solvents ensures uniform distribution of the solute.

(174) The nonaqueous solvent was chosen for its ability to dissolve the polar solute.

(175) The molal concentration of the solute was determined using a cryoscopic method.

(176) The desolvation of a solute can result in the formation of a solid precipitate.

(177) The number of solute particles determines the extent of colligative properties.

(178) The isopiestic method was used to determine the molecular weight of the solute.

(179) Solvation is the process of surrounding solute particles with solvent particles.

(180) The solute concentration in the solution was measured using a spectrophotometer.

(181) Plasmolysis is more likely to occur in cells with a higher solute concentration.

(182) The volumetric analysis of the solution revealed a high concentration of solute.

(183) The desolvation process involves the removal of solvent molecules from a solute.

(184) The desolvation of a solute can be a slow process that requires careful control.

(185) The solvation of a solute can lead to the stabilization of its ions in solution.

(186) The miscibility of a solute in a solvent affects the solubility of the solution.

(187) The solute particles reacted with the solvent in solution to form a new compound.

(188) The desolvation of a solute can be monitored using various analytical techniques.

(189) The manometrically determined concentration of the solute was 0.5 moles per liter.

(190) The molality of a solution can be altered by adding or removing solute or solvent.

(191) The physicochemical properties of the solvent affect the solubility of the solute.

(192) The process of endosmose is influenced by the size and charge of solute particles.

(193) The concentration of the solute in solution was too high for accurate measurement.

(194) The solvation of a solute can be visualized using techniques such as spectroscopy.

(195) The solvation of a solute can result in the formation of solute-solvent complexes.

(196) The solvation process can be influenced by the polarity of the solute and solvent.

(197) The equimolar solution was prepared by adding equal amounts of solute and solvent.

(198) The vapour-pressure of a solution depends on the concentration of solute particles.

(199) The molarity of the solution was calculated based on the number of moles of solute.

(200) The unsaturated solution was heated to evaporate the solvent and obtain the solute.

(201) The osmolarity of a solution can be altered by adding or removing solute particles.

(202) The process of endosmosis is influenced by the size and charge of solute particles.

(203) The cooling of the solution caused the solute to precipitate out and form crystals.

(204) Supersaturation is a delicate balance between solute concentration and temperature.

(205) The desolvation of a solute can be influenced by the concentration of the solution.

(206) The conductibility of a solution can be decreased by adding a non-conductive solute.

(207) The dissolvability of the solute in the solvent is affected by the pressure applied.

(208) The molal concentration of the solute was affected by the presence of other solutes.

(209) Solvation is an important factor in determining the rate of dissolution of a solute.

(210) The vapour-pressure of a solution decreases as the concentration of solute increases.

(211) The concentration of the solute in solution was determined using a spectrophotometer.

(212) The colligative properties of a solution are affected by the concentration of solute.

(213) The colligative properties of a solution are independent of the nature of the solute.

(214) The solubilization process can be optimized by adjusting the solvent-to-solute ratio.

(215) The nonaqueous solution was prepared by dissolving the solute in the organic solvent.

(216) The isocline of the concentration gradient shows areas of equal solute concentration.

(217) The molal concentration of the solute was too low to observe any significant effects.

(218) The dissolubility of the solute in the solvent can be increased by adding a catalyst.

(219) Solvation is a process that occurs spontaneously when a solute is added to a solvent.

(220) The cooling of a supersaturated solution causes the excess solute to crystallize out.

(221) The refractivities of the solutions were affected by the concentration of the solute.

(222) Supersaturation can be achieved by cooling a solution or by adding more solute to it.

(223) The solution became supersaturated when more solute was added than could be dissolved.

(224) The desolvation of a solute can lead to changes in its solubility and bioavailability.

(225) The desolvation of a solute can be enhanced by using techniques such as freeze-drying.

(226) The absorbance of the solution decreased as the concentration of the solute decreased.

(227) The solubilization of a solute in a solvent can result in the formation of a solution.

(228) The solute particles diffused from an area of high concentration to low concentration.

(229) The molar concentration of a solution can be altered by adding more solute or solvent.

(230) The concentration of a solute in an aqueous solution can be expressed as a percentage.

(231) The isopiestic nature of these solutions allows for the prediction of solute movement.

(232) The formation of crystals occurs when a liquid solution becomes saturated with solute.

(233) The molal activity coefficient of the solute in the solution was determined to be 0.8.

(234) To supersaturate a solution, you need to add more solute than the solvent can dissolve.

(235) The solvation of a solute can be enhanced by increasing the surface area of the solute.

(236) The diffusivity of a solute in a polymer matrix can be enhanced by adding plasticizers.

(237) As you rarefy the solution, you will notice the concentration of the solute decreasing.

(238) The cooling of the solution caused the solute to precipitate out and form a precipitate.

(239) The strength of molecular attraction influences the solubility of a solute in a solvent.

(240) The maximum density of the solution was obtained by adding the precise amount of solute.

(241) The chemist was able to supersaturate the solution by heating it and adding more solute.

(242) The solute particles interacted with the solvent molecules through intermolecular forces.

(243) The molality of a solution can be used to determine the activity coefficient of a solute.

(244) The solution was heated to a specific temperature to encourage the solute to crystallize.

(245) The molal concentration of the solute was found to be constant at different temperatures.

(246) The chemist attempted to supersaturate the solution by heating it and adding more solute.

(247) The solution was heated to a specific temperature to encourage the solute to crystallise.

(248) The colligative properties of a solution depend on the concentration of solute particles.

(249) Adding a solute to a solvent alters the colligative properties of the resulting solution.

(250) The desolvation of a solute can result in changes in its physical and chemical properties.

(251) The colligative properties of a solution depend on the number of solute particles present.

(252) Osmotic flow is driven by the difference in solute concentration between two compartments.

(253) Increasing the molar concentration of a solute can affect the rate of a chemical reaction.

(254) The molar concentration of a solution can be used to calculate the solubility of a solute.

(255) The molal concentration of the solute was converted to molar concentration for comparison.

(256) The densimetric data can be used to calculate the concentration of a solute in a solution.

(257) The vapour-pressure of a solution can be affected by the addition of a non-volatile solute.

(258) The desolvation of a solute can be affected by the size and shape of the solvent molecules.

(259) The solvation shell around a solute molecule consists of solvent molecules attracted to it.

(260) The colligative properties of a solution are influenced by the solvent-solute interactions.

(261) The concentration of a solution is directly proportional to the amount of solute dissolved.

(262) The process of exosmosis is influenced by the size of the solute particles in the solution.

(263) The dissolvability of the solute in the solvent is crucial for the formation of a solution.

(264) The dissolvability of the solute in the solvent is influenced by the size of the particles.

(265) The vapour-pressure of a solution can be influenced by the nature of the solute and solvent.

(266) The desolvation of a solute can be influenced by the presence of other solutes or additives.

(267) The desolvation of a solute can be controlled by adjusting the concentration of the solvent.

(268) The desolvation of a solute can be influenced by the presence of surfactants or stabilizers.

(269) The absorbance of the solution was directly proportional to the concentration of the solute.

(270) The enthalpy of hydration is the heat released or absorbed when a solute dissolves in water.

(271) The dissolvability of the solute in the solvent is influenced by the presence of impurities.

(272) The molal concentration of the solute in the solution was too high for accurate measurement.

(273) The molal concentration of the solute was found to be inversely proportional to temperature.

(274) The dissolubility of the solute in the solvent determines the concentration of the solution.

(275) The undersaturated solution had a lower concentration of solute than the saturated solution.

(276) The nonaqueous solution was stirred vigorously to ensure complete dissolution of the solute.

(277) The supersaturated solution was carefully mixed to ensure uniform distribution of the solute.

(278) Adding a solute to a solvent can change the colligative properties of the resulting solution.

(279) The colligative properties of a solution can be used to determine the molar mass of a solute.

(280) Osmotic regulation in bacteria involves the control of solute concentration in the cytoplasm.

(281) The dissolubility of the solute in the solvent can be affected by the presence of impurities.

(282) The solvation of a solute can be influenced by the presence of other solutes in the solution.

(283) The supersaturated solution was carefully decanted to separate it from any undissolved solute.

(284) The colligative properties of a solution are only dependent on the number of solute particles.

(285) Adding a non-volatile solute to a solvent increases its boiling point, a colligative property.

(286) The solution became supersaturated when more solute was added than the solvent could dissolve.

(287) The solvation of a solute can be influenced by the concentration of the solute in the solvent.

(288) If you introduce a solute molecule to a solvent, it can change the properties of the solution.

(289) The colligative properties of a solution are affected by the type of solute particles present.

(290) The supersaturated state of the solution was achieved by adding the solute in small increments.

(291) The colligative properties of a solution are affected by the concentration of solute particles.

(292) The molality of a solution is defined as the number of moles of solute per kilogram of solvent.

(293) The molality of a solution can be used to calculate the osmotic pressure exerted by the solute.

(294) The enthalpy of solution is the heat absorbed or released when a solute dissolves in a solvent.

(295) The molal concentration of the solute was found to be independent of the volume of the solvent.

(296) The liquefacient was added to the solvent to increase its ability to dissolve the solid solute.

(297) The gelation behavior of a solution can be altered by changing the concentration of the solute.

(298) The molar concentration of the solute in the solution was determined using a spectrophotometer.

(299) The colligative properties of a solution are independent of the chemical identity of the solute.

(300) The molar concentration of a solute can be used to calculate the osmotic pressure of a solution.

(301) The osmolar pressure of a solution can be affected by changes in the number of solute particles.

(302) The paper proposed a semiempirical equation to describe the diffusion coefficient of the solute.

(303) The dissolvability of the solute in the solvent is affected by the presence of other substances.

(304) The dissolubility of the solute in the solvent can be decreased by adding a precipitating agent.

(305) The solvation of a solute can be influenced by the presence of other substances in the solution.

(306) The process of super-saturation occurs when a solution contains more solute than it can dissolve.

(307) The molar concentration of a solution can be used to determine the rate of diffusion of a solute.

(308) The molal concentration of the solute was used to calculate the osmotic pressure of the solution.

(309) The colligative properties of a solution are influenced by the concentration of solute particles.

(310) The supersaturated solution exhibited a higher concentration of solute than its saturation point.

(311) The Sherrington equation is used to calculate the diffusion coefficient of a solute in a solvent.

(312) The colligative properties of a solution are influenced by the number of solute particles present.

(313) The dissolubility of the solute in the solvent can be influenced by the presence of other solutes.

(314) Solvation is a dynamic process that involves the interaction between solute and solvent molecules.

(315) The supersaturated solution contained more solute than it could normally hold at that temperature.

(316) The colligative properties of a solution are influenced by the size and shape of solute particles.

(317) The chemicophysical properties of the solution were influenced by the concentration of the solute.

(318) The liquid-phase diffusion of the solute through the membrane was studied using a permeation cell.

(319) Solvation is a dynamic process where solvent molecules continuously interact with solute particles.

(320) The colligative properties of a solution can be used to determine the molecular weight of a solute.

(321) The dissolvability of the solute in the solvent is influenced by the concentration of the solution.

(322) The colligative properties of a solution are proportional to the concentration of solute particles.

(323) The cooling of a supersaturated solution causes the excess solute to crystallize, forming crystals.

(324) The colligative properties of a solution are affected by the size and shape of the solute particles.

(325) The molar concentration of a solution can be used to determine the activity coefficient of a solute.

(326) The molal concentration of the solute was determined by measuring the boiling point of the solution.

(327) The solubility of a solute in a solvent will remain constant at a specific temperature and pressure.

(328) Turgor loss can occur due to a decrease in water availability or an increase in solute concentration.

(329) The osmotic pressure of a solution is directly proportional to the concentration of solute particles.

(330) The process of exosmosis is affected by the presence of solute particles in the surrounding solution.

(331) The process of exosmosis is affected by the pressure exerted by the solute particles in the solution.

(332) The molal concentration of the solute was determined by measuring the freezing point of the solution.

(333) The volumetrical calculations were used to determine the concentration of the solute in the solution.

(334) The colligative properties of a solution are affected by the size and charge of the solute particles.

(335) The colligative properties of a solution are influenced by the size and shape of the solute particles.

(336) The solute particles of nitrogen began to dissolve as soon as they came into contact with the solvent.

(337) The osmose of water into a cell can cause it to swell or shrink depending on the solute concentration.

(338) The boiling point elevation is a colligative property that increases with the concentration of solute.

(339) The vapor pressure lowering is a colligative property that decreases with the concentration of solute.

(340) The refractometry measurements are often used to calculate the concentration of a solute in a solution.

(341) The absorbance of the solution was found to be directly proportional to the concentration of the solute.

(342) Osmotic pressure is a colligative property that depends on the number of solute particles in a solution.

(343) Supersaturation occurs when a solution contains more solute than it can dissolve at a given temperature.

(344) The freezing point depression is a colligative property that decreases with the concentration of solute.

(345) The colligative properties of a solution can be used to calculate the degree of dissociation of a solute.

(346) The supersaturated solution was carefully heated to remove excess solute and stabilize its concentration.

(347) To create a supersaturated solution, you need to dissolve more solute than the solvent can normally hold.

(348) The molarity of the solution was determined by dividing the moles of solute by the volume of the solution.

(349) The molarity of the solution was calculated based on the mass of the solute and the volume of the solvent.

(350) The supersaturated solution was prepared by dissolving excess solute in a hot solvent and then cooling it.

(351) The process of super-saturation occurs when a solution contains more solute than it can normally dissolve.

(352) Supersaturation can be achieved by cooling a solution slowly and allowing excess solute to precipitate out.

(353) The colligative properties of a solution can be used to determine the molecular weight of an unknown solute.

(354) The supersaturated solution was created by dissolving a large amount of solute in a small amount of solvent.

(355) The molal concentration of the solute was determined by measuring the colligative properties of the solution.

(356) The molal concentration of the solute was lower in the dilute solution compared to the concentrated solution.

(357) Hydrotropic interactions occur between the hydrotropic agent and the solute, leading to increased solubility.

(358) Supersaturation occurs when a solution contains more solute than it can normally hold at a given temperature.

(359) The osmotic pressure of a solution is a colligative property that increases with the concentration of solute.

(360) The molality of a solution can be determined by weighing the solvent and measuring the amount of solute added.

(361) The molal concentration of the solute was higher in the concentrated solution compared to the dilute solution.

(362) The supersaturated solution was prepared by adding more solute to the solvent than it could normally dissolve.

(363) The supersaturated solution was highly concentrated and had a solute concentration above its saturation point.

(364) The equilibrium constant can be used to determine the distribution of a solute between two immiscible solvents.

(365) Osmotic pressure can cause water to move from an area of low solute concentration to high solute concentration.

(366) The boiling point of a solution is a colligative property that increases with the addition of solute particles.

(367) The kidneys play a vital role in osmoregulation by filtering and regulating the body's water and solute levels.

(368) The decinormal solution was prepared by dissolving a specific amount of solute in a specific volume of solvent.

(369) The absorbance of the solution was plotted against the concentration of the solute to create a calibration curve.

(370) The key to creating a supersaturated solution is to carefully control the temperature and amount of solute added.

(371) The constant of proportionality between the amount of solute and the concentration is the volume of the solution.

(372) The molality of the solution was used to determine the amount of solute needed to prepare a specific concentration.

(373) The colligative properties of a solution are a result of the interactions between the solute and solvent particles.

(374) The supersaturated solution was created by adding more solute to the solvent than it could hold at that temperature.

(375) The molal concentration of the solute was found to be directly proportional to the number of moles of solute present.

(376) Exosmosis is a slow process compared to endosmosis due to the higher concentration of solute particles inside the cell.

(377) The concept of colligative properties is based on the idea that solute particles disrupt the solvent's normal behavior.

(378) The supersaturated solution was highly concentrated and had a higher solute-to-solvent ratio than its saturation point.

(379) The supersaturated solution was carefully prepared by dissolving the solute in a hot solvent and then cooling it slowly.

(380) If there is a high concentration of solute outside the cell, active transport may be necessary to move molecules inside.

(381) The supersaturated solution was achieved by cooling the solution slowly to allow for the excess solute to remain dissolved.

(382) The supersaturated solution was prepared by heating the solvent and then adding excess solute until no more could dissolve.

(383) The concentration of a chemical in a solution is a continuous variable that can vary depending on the amount of solute present.

(384) Supersaturation can be achieved by cooling a solution slowly, allowing more solute to dissolve than would normally be possible.

(385) Osmotic pressure is a phenomenon that occurs when there is a difference in solute concentration across a semipermeable membrane.

(386) The supersaturated solution was formed by dissolving more solute in the solvent than it could normally hold at that temperature.

(387) The concentration of a solute in a solution is often proportional to the amount of solute dissolved in a given volume of solvent.

(388) Hydrotropic effects can be influenced by the physicochemical properties of the solute, such as its molecular weight or lipophilicity.

(389) The process of supersaturation involves reaching a state where the solution is holding more solute than it should be able to dissolve.

(390) The supersaturated solution was achieved by dissolving a large amount of solute in a small amount of solvent and then cooling it slowly.

(391) The supersaturated solution was achieved by dissolving a large amount of solute in a small amount of solvent and then slowly cooling it.

(392) The supersaturated solution was formed by heating the solvent and then slowly cooling it to allow for the excess solute to remain dissolved.

(393) The supersaturated solution was carefully prepared by dissolving the solute in a hot solvent and then filtering out any undissolved particles.

(394) The supersaturated solution was prepared by heating the solvent and then adding excess solute until no more could dissolve, followed by slow cooling.

(395) The process of osmosis occurs when there is a difference in solute concentration across a membrane, and an isosmotic solution prevents this from happening.

(396) The osmotic pressure of a solution is directly proportional to the concentration of solute particles in the solution, and it can be calculated using the van't Hoff equation.

(397) Osmotic pressure is a phenomenon that occurs when a solute is dissolved in a solvent, causing the solvent to move from an area of low concentration to an area of high concentration.

(398) The phenomenon of osmosis is a physical process where water molecules move across a semipermeable membrane from an area of lower solute concentration to an area of higher solute concentration.

(399) The phenomenon of osmosis is a physical process in which solvent molecules pass through a semipermeable membrane from an area of low solute concentration to an area of high solute concentration.

(400) When a cell is placed in a hypertonic solution, meaning the solute concentration outside the cell is higher than inside, water will move out of the cell through osmosis, causing the cell to shrink.

(401) Osmotic pressure is a phenomenon that occurs when two solutions of different concentrations are separated by a semipermeable membrane, and it can cause water to move from an area of low solute concentration to an area of high solute concentration.

The word usage examples above have been gathered from various sources to reflect current and historical usage of the word Solute. They do not represent the opinions of TranslateEN.com.