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2. A solution is made as follows: 2.735g of Ca(NO3)2 is dissolved in 1.000L of distilled...
2. A solution is made as follows: 2.735g of Ca(NO), is dissolved in 1.000L of distilled deionized water. What is the molar solubility of Ag,SO, in this solution of Ca(NO)? The pk., value of Ag,SO, is 4831. (Hint: You may need to write the equilibrium expression in terms of activities and ignore the contribution to ionic strength from Ag.SO.) (10 points)
1. 25.00 mL of a of 0.100M solution of formic acid (HCO,H, PK, = 3.74) is titrated with 0.125 Min NaOH. What is the pH at each of the following? (5 points each) a. After the addition of 15.00mL of NaOH solution. b. After the addition of 20.00 mL of NaOH solution c. After the addition of 25.00 mL of NaOH solution. d. At what volume of added NaOH will pH =pK. 2. A solution is made as follows: 2.735g...
1A) How will the calculated Ksp value of Ca(OH)2 be affected if the original Ca(OH)2 solution is not saturated? Explain? B) Does adding distilled water to the titrating flask in order to wash the sides of the flask and the buret tip affect the computed Ksp of Ca(OH)2? Explain? C) How might tap water instead of distilled water affect the calculated Ksp of Ca(OH)2? Explain? D) The temperature of the solution was 21.1 degrees Celcius. Is the molar solubility of...
Calculate the molar solubility of CaF2 in a solution containing 0.871 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units. S =
calculate the ph, ph=-log(AH+) of a 0.0200 M solution of Ca(NO3)2 to which 5.87 x10^-7 moles of HCL have been added per L of solution. Include ionic strength effects in this calculation and equilibrium constant.
Calculate the molar solubility of CaF2 in a solution containing 0.357 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units.
During a water treatment program, 127 grams of calcium nitrate, Ca(NO3)2, is dissolved in water. The final volume of the solution is 2,300 milliliters. What is the molarity of the solution?
When solid Ca(CH3COO)2 is dissolved in a nearly saturated solution of Ca(CH3COO)2 the solution becomes warmer. This information indicates that if the temperature of asolution is decreased,a. delta H will become zerob. the solubility of Ca(CH3COO)2 will increasec. delta H will become negatived. the solubility of Ca(CH3COO)2 will decreasee. the solubility of Ca(CH3COO)2 will not change
Calculate the molar solubility of CaF2 in a solution containing 0.647 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units.
b. MgCl, is dissolved in distilled water at 25°C until the saturated solution is obtained (system reaches equilibrium). The concentration of Mg2 in the saturated solution is 1.35 x 10-'M. The dissolution of MgCl, in distilled water is endothermic. Write the balanced chemical equation to obtain the saturated solution Calculate the solubility product, K of MgCl2. Explain the effect of increasing the temperature on the amount of MgCl, Justify your answer. C. When solid Pbl, is added to pure water...