Q: The molar solubility of lead chromate in a 0.250 M ammonium chromate solution is
A:
Q: The molar solubility of calcium fluoride in a 0.129 M sodium fluoride solution is M
A:
Q: The molar solubility of lead chromate in a 0.266 M lead nitrate solution is M.
A: in presence of strong electrolyte, solubility of weak electrolyte decreases.
Q: The molar solubility of lead chromate In a water solutlon is M.
A:
Q: The molar solubility of lead iodide in a 0.139 M lead acetate solution is M.
A: Given : Concentration of Lead acetate i.e Pb(CH3COO)2 = 0.139 M Since Pb(CH3COO)2 is a completely…
Q: What is the solubility product constant for
A: We will calculate Ksp
Q: The molar solubility of lead bromide in a 0.119 M lead nitrate solution is __ M
A: Since in lead nitrate the reaction will be Pb(NO3)2 ----> Pb2+ + 2NO32- Since lead nitrate is…
Q: The molar solubility of calcium fluoride in a 0.274 M calcium acetate solution is ______M.
A:
Q: The molar solubility of calcium phosphate in a water solution is. M
A: The given compound is Ca3(PO4)2.
Q: The molar solubility of barium fluoride in a 0.210 M sodium fluoride solution is M.
A:
Q: The molar solubility of cobalt(II) sulfide in a 0.220 M sodium sulfide solution is
A: Let assume that molar solubility of Cobalt(II) sulfide as S mol/litre The dissociation of Cobalt(II)…
Q: Calculate the solubility (in g/L) of strontium phosphate, Sr3(PO4)2. The Ksp is 4E-28, and its molar…
A: SOLUBILITY :- The maximum mass of solute particle that can be dissolved in a given amount of…
Q: The molar solubility of barium fluoride in a 0.142 M ammonium fluoride solution is М.
A:
Q: The molar solubility of silver chloride in a water solution is M.
A: Molar solubility of AgCl in water Ksp = [Ag+][Cl-] = 1.8 x 10^-10 let x amount of AgCl is in…
Q: The molar solubility of calcium hydroxide in a water solution is ]M.
A: To calculate molar solubility of Ca(OH)2 in water Solubility product constant of calcium hydroxide…
Q: The molar solubility of calcium hydroxide in a water solution is M.
A: Molar solubility of calcium hydroxide can be calculated as follows
Q: The molar solubility of lead phosphate in a 0.291 M ammonium phosphate solution is |M.
A: The question is based on the concept of common Ion effect. it states that solubility of weak…
Q: The molar solubility of manganese(II) sulfide in a 0.115 M manganese(II) acetate solution is М.
A: The molar solubility of MnS in a 0.115 M Manganese(II)acetate is 0.115 M.
Q: The molar solubility of lead chromate in a 0.254 M lead nitrate solution is| M.
A: given we have 0.254 M solution of lead nitrate which means; We have balanced chemical reaction for…
Q: The molar solubility of lead chromate in a 0.214 M potassium chromate solution is M.
A:
Q: The molar solubility of iron(II) sulfide in a 0.168 M potassium sulfide solution is |M.
A:
Q: What is the solubility(in mol/L) of magnesium hydroxide?
A: Magnesium hydroxide is sparingly soluble salt in water. It is very slightly soluble in water. Ions…
Q: The molar solubility of silver sulfate in a 0.152 M potassium sulfate solution is М.
A: Given: Concentration of potassium sulfate K2SO4 is 0.152 M K2SO4-------> 2K+ (aq) + SO42- So,…
Q: The molar solubility of silver chromate in a 0.258 M sodium chromate solution is ?
A: Solubility product of silver chromate (Ag2CrO4) is Ksp=1.1×10-12 (Standard value) Dissociation…
Q: The molar solubility of barium sulfate in a 0.175 M barium acetate solution is what? (M)
A: Solubility product (Ksp) defines any component’s solubility. Highly soluble components possess…
Q: The molar solubility of cobalt(II) hydroxide in a 0.223 M cobalt(II) nitrate solution is M.
A:
Q: Addition of Lead nitrate water solution to weak solution of Potassium chloride leads to…
A: The correct option is option (1) C(Pb+2).C2(Cl-)>Kos(PbCl2)
Q: he molar solubility of lead sulfate in a 0.101 M lead nitrate solution is
A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…
Q: intermolecular force causes the dissolution of FeCl, in water
A:
Q: The molar solubility of magnesium hydroxide in a 0.280 M magnesium acetate solution is М.
A: Solubility is defined as the maximum amount of solute that can be dissolved in a solvent at…
Q: The maximum amount of barium sulfite that will dissolve in a 0.271 M potassium sulfite solution is…
A: Given : Potassium sulfite = 0.271 M
Q: The molar solubility of zinc phosphate in a 0.172 M potassium phosphate solution is ___ M.
A:
Q: Calculate the AH(dissolve) for oxygen solubility in water, in kJ/ mol.
A: The relationship between equilibrium constant and ∆H with temperature change is calculated below.
Q: a. What is the molar solublity of lead(II) chloride in water?b. Should we be concerned about the…
A: a) Since the solubility product of PbCl2 is = 1.7 X 10-5 Reaction taking place => PbCl2 ---->…
Q: The molar solubility of magnesium fluoride in a 0.268 M potassium fluoride solution is M.
A: Given: Molarity of potassium fluoride solution = 0.268 M Known: Ksp of magnesium fluoride = 6.5×10-9
Q: Is the following compound solid or aqueous compound? using the solubility table NH4Br
A: A neutralization reaction involves the reaction of an acid with a base to form salt and water.…
Q: The molar solubility of Barium hydroxide is 0.1077 M, what is the Ksp?
A:
Q: The molar solubility of barium phosphate in a 0.222 M barium nitrate solution is M.
A: The concentration of barium nitrate, Ba(NO3)2 = 0.222 M
Q: The molar solubility of zinc carbonate in a water solution is M.
A: Molar solubility is directly related to the solubility product and it is defined as number of moles…
Q: What is the solubility of ammonia in water in moles per liter?
A: Solubility of any substance in a solvent may be defined as the number of moles of that substance…
Q: The molar solubility of calcium sulfate in a 0.147 M calcium nitrate solution is M.
A: The dissociation reaction for CaSO4 in water is shown below, CaSO4⇌Ca2+(aq)+SO42-(aq) The Ksp…
Q: The molar solubility of zinc phosphate in a water solution is М.
A: The molar solubility tells about the amount of solute that can be made to get dissolved in a liter…
Q: The solubility of magnesium fluoride, , in water is 1.5x10^-2 g/L. What is the solubility (in grams…
A:
Q: solution (100 mL) containing 325 ppm K+ is analyzed by precipitating it as the tetraphenyl borate,…
A:
Q: Define the term Solubility Product Constant?
A: Solubility is defined as a property of a substance called solute to get dissolved in a solvent in…
Q: The molar solubility of lead bromide in a 0.207 M sodium bromide solution is M.
A:
Q: The molar solubility of aluminum phosphate in a 0.183 M sodium phosphate solution is М.
A:
Q: The maximum amount of magnesium fluoride that will dissolve in a 0.290 M magnesium nitrate solution…
A: Ksp of MgF2 at 25o C is 6.5×10-9. MgF2 dissociates as follows: Let the solubility of [Mg2+] be ‘s’.…
Q: The molar solubility of silver sulfate in a 0.148 M potassium sulfate solution is M.
A: Solubility is the relative extent of a solute to dissolve into a solvent. Therefore, molar…
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- A 0.010 M solution of the weak acid HA has an osmotic pressure (see chapter on solutions and colloids) of 0.293 atm at 25 C. A 0.010 M solution of the weak acid HB has an osmotic pressure of 0.345 atm under the same conditions. (a) Which acid has the larger equilibrium constant for ionization HA[HA(aq)A(aq)+H+(aq)] or HB[HB(aq)H+(aq)+B(aq)]? (b) What are the equilibrium constants for the ionization of these acids? (Hint: Remember that each solution contains three dissolved species: the weak acid (HA or HB). the conjugate base (A- or B- and the hydrogen ion (H+). Remember that osmotic pressure (like all colligative properties) is related to the total number of solute particles. Specifically for osmotic pressure, those concentrations are described by molarities.)Figure 16.3 shows the solubility of AgNO3 in water inunits of moles of AgNO3 per kilogram of H2O. If 255 g of AgNO3 is added to 100 g of water at 95°C and cooledslowly, at what temperature will the solution becomesaturated?A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal placesA solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)
- A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)1.0 GRAMS of an electrolyte was dissolved in 29 grams of water, the resulting solution was found to have a molarity of 0.437 mol / L. The freezing point of the solution was determined to be -4.96°C. The freezing point depression constant for water is -1.86°C and pure water may be assumed to freeze at 0°C. If the molecular weight of the electrolyte is 179.7 g/mol and it takes 15 minutes to perform the experiment, how much water was used (grams) ?Solubility tests of benzoic acid with a dissolution enthalpy of -32kJ / mol were performed at 2 different temperatures. In the first experiment carried out at 27 ° C, 5 mL of the sample taken from the benzoic acid solution is taken into 25 mL of water and titrated with 0.02M NaOH. As a result of the titration, there is a consumption of 8 mL, respectively. In the second experiment performed at a different temperature under the same conditions, 22 mL was consumed. Taking advantage of these results a) Solubility of benzoic acid at 27 ° C .................................................; b) solubility of benzoic acid at different temperature ................................................; c) second test temperature ....................................................... (M (benzoic acid): 122.12 g / mol) Note: enter only required numerical values and units in the spaces in the question.
- 23. The Ksp of CuCO3ls) (copper carbonate, a salt) is reported as 2.21x10-11. Determine the solubility (in mg/L) of 1this salt in pure water Constants: The molecular mass (M) of copper carbonate (CuCOg) is 123.554 g mol-1I would like to calculate the molar solubility and Ksp from the following data: I have calculated them (see the solutions in the table) but, I am concerned that I have done the calculation incorrectly. See images for my calculations. These calculations are for Sample 1. Thank you! Sample 1 Sample 2 Sample 3 Mass of Erlenmeyer Flask 23.59g 23.59g 23.60g Mass of Erlenmeyer Flask + Calcium Hydroxide Solution (lime water) 26.62g 26.65g 26.69g Mass of Calcium Hydroxide Solution 3.03g 3.06g 3.09g Volume of Ca(OH)2 Density = 1.000 g/mL 3.03mL 3.06mL 3.09mL Concentration of HCl (M) 0.1M 0.1M 0.1M Initial HCl Volume in Syringe 1.00mL(1) 1.00mL(2) 1.00mL(3) 1.00mL(1) 1.00mL(2) 1.00mL(3) 1.00mL(1) 1.00mL(2) 1.00mL(3) Final HCl Volume in Syringe 0ml (1) 0ml (2) 0.65mL (3) 0ml (1) 0ml (2) 0.63mL (3) 0ml (1) 0ml (2) 0.63mL (3) Volume of HCl Delivered 2.35mL 2.37mL 2.37mL Moles of HCl Delivered…Which of the following compounds will be the MOST soluble in pure water at 25 ˚C? A. Lead (II) carbonate, PbCO3 Ksp = 7.4×10–14 B. Cobalt (II) carbonate, CoCO3 Ksp = 1.4×10–13 C. Manganese (II) carbonate, MnCO3 Ksp = 1.8×10–11 D. Cadmium carbonate, CdCO3 Ksp = 5.2×10–12 E. Barium carbonate, BaCO3 Ksp = 5.1×10–9