(a)
Interpretation:
The net reaction of dissolution of
Concept introduction:
Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by
The expression for its
A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant
The relation between
(b)
Interpretation:
The net reaction of dissolution of
Concept introduction:
Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by
The expression for its
A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant
The relation between
(c)
Interpretation:
The net reaction of dissolution of
Concept introduction:
Solubility product is equilibrium constant for reactions that occur when an ionic compound is dissolved to produce ions. It is denoted by
The expression for its
A complex ion is ion that contains a metal cation bonded to one or more small ions. The formation of complex ion is generally a stepwise procedure and each step has its equilibrium constant. The stability of complex ion is measured by formation constant
The relation between
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Chemistry, Loose-leaf Edition (8th Edition)
- (7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.arrow_forward(a) Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoic acid (C6H5COOH, Ka = 6.3 * 10-5). (b) Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.arrow_forward(a) Calculate the pH in the solution formed by adding10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoicacid (C6H5COOH, Ka = 6.3 x 10-5). (b) Calculate the pHin the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.arrow_forward
- The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forwardWhich of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)arrow_forward4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.arrow_forward
- Consider the titration of formic acid, HCHO2, with barium hydroxide. (a) Write a balanced net ionic equation for the reaction. (b) Calculate K for the reaction. (c) Is the solution at the equivalence point acidic, basic, or neutral? (d) What would be an appropriate indicator for the titration?arrow_forward1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the following changes are made to a saturated solution, what will be the effect on the [Ca2+]? Ca(OH)2 (s) <--> Ca2+(aq) + 2 OH- (aq) ΔH = -16.6 kJ A strong base is added to the solution (Decrease, Increase, No change) More solid Ca(OH)2 is added to the container (Decrease, Increase, No change) The solution is raised to a higher temperature (Decrease, Increase, No change) A strong acid is added to the solution (Decrease, Increase, No change) Ca(NO3)2 (s) is added. Ca(NO3)2 is very soluble (Decrease, Increase, No change)arrow_forwardA 500.-mL solution consists of 0.050 mol of solid NaOH and 0.13 mol of hypochlorous acid (HClO; Kₐ=3.0X10⁻⁸) dis-solved in water.(a) Aside from water, what is the concentration of each species that is present?(b) What is the pH of the solution?(c) What is the pH after adding 0.0050 mol of HCl to the flask?arrow_forward
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