Based upon the chemical equilibrium reaction shown below explain what will happen in each scenario a

1. How many moles of Ca2+ and OH- ions are produced for every one mole of Ca(OH)2 that dissolves in solution? Ca(OH)2(s)↔ Ca2+(aq) + 2OH-(aq)   2. A student determined that 20.0 mL of a saturated calcium hydroxide solution required 5.23 mL of a 0.108 M HCl solution to reach the equivalence point. Calculate the number of moles of Ca(OH)2 titrated and the molar concentration of the saturated Ca(OH)2 solution. Ca(OH)2(aq)+ 2HCl (aq)→ CaCl2(aq) + 2H2O(l)   3. Calculate the Ksp of Ca(OH)2

. CO2 + 2 NH2OH CO + N2 +3 H2O in basic solution

A solution contains both NaHCO3 and Na2CO3. Titration of a 50.00 mL portion to a phenolphthalein end point requires 21.25 mL of 0.1385 M HCl. A second 50.00 mL aliquot requires 45.48 mL of the HCl solution when titrated to a bromocresol green end point. Calculate the molar concentration of Na2CO3 in the original solution. (Do not include the unit for molarity. Enter your answer to three significant figures.)

6. Both CO3 and HCO3 respond to the usual carbonate ion test. Give specific procedures by which you could distinguish between these ions in an unknown. (Hint: Consider the pH of the solution.) 2-

Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A

Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture of NaHCO3 and Na2CO3 was titrated, what would be the relative sizes of V1, and V2? b. If a mixture of NaOH and Na2CO3 was titrated, what would be the relative sizes of V1 and V2? c. A sample contains a mixture of NaHCO3 and Na2CO3. When this sample was titrated with 0.100 M HCl, it took 18.9 mL to reach the first stoichiometric point and an additional 36.7 mL to reach the second stoichiometric point. What is the composition in mass percent of the sample?

A few drops of each of the indicators shown in the accompanying table were placed in separate portions of a 1.0-M solution of a weak acid, HX. The results are shown in the last column of the table. What is the approximate pH of the solution containing HX? Calculate the approximate value of Ka for HX. Indicator Color of Hln Color of ln pKa of Hln Color of 1.0 M HX Bromphenol blue Yellow Blue 4.0 Blue Bromcresol purple Yellow Purple 6.0 Yellow Bromcresol green Yellow Blue 4.8 Green Alizarin Yellow Red 6.5 Yellow

A 0.250 M solution of a weak base R2NH has a pH of 10.60 at 25C. What is G for the dissociation of the weak base in water at 25C? R2NH(aq)+H2OR2NH2+(aq)+OH(aq)

1. Calculate the pH of a 0.048 M solution of NaCH3COO. (Sodium acetate) [4]