Write an equation for the reaction of each of the following with water a) HCl b)

Question

Write an equation for the reaction of each of the following with water a) HCl b) H_2SO_4 c) HCOOH d) NaOH e)NH_3 Identify the conjugate acid-base pairs in each of the following chemical reactions: a) NH^+_4 (aq) + CN^-(aq) NH_3(aq) + HCN(aq) b) CO^2-_3 (aq) + HCl(aq) HCO^-_3 (aq) + Cl^-(aq) c) HCl(aq) + OH^-(aq) H_2O(aq) + Cl^-(aq) Classify each of the following as Bronsted acid, Bronsted base, or both in aqueous solution: a) H_2O b) H_2SO_4 c) HSO^-_4 d) SO^2-_4 e) NH^+_4 f) NH_3 g) CH_3COO^- (acetate ion) Calculate the pH of a solution that is: a) 1.0 times 10^-4 M in HCl b) 1.0 times 10^-3 M in NaOH Calculate both [H_3O^+] and [OH^-] for a solution for which: a) pH - 6.30 b) pH - 1.70 c) pH - 5.50 d) pH - 7.00 Write the net ionic equation to represent the neutralization of an aqueous solution of HCl with an aqueous solution of NaOH. Which of the following are capable of forming a buffer solution? Which of the following are capable of forming a buffer solution? a) NH_3 and NH_4Cl b) HNO_3 and KNO_3 c) HBr and MgCl_2 d) H_2CO_3 and NaHCO_3 What is [H_3O^+] for a buffer solution that is 0.100 M in acid and 0.100 M in the corresponding salt if the weak acid ka = 5.80 times 10^-7? The pH of blood plasma is 7.40. The principal buffer system is HCO^-_3/H_2CO_3. Calculate the ratio [HCO^-_3]/[H_2CO_3] in blood plasma. (K_a of H_2CO_3, carbonic acid, is 4.45 times 10^-7.)

Explanation / Answer

Q1.

dissociation:

a)

HCl(aq) + H2O(l) --> H3O+(aq) + Cl-(aq)

b)

H2SO4(aq) + 2H2O(l) -> 2H3O+(aq) + SO4-2(aq)

c)

HCOOH(aq) + H2O(l) ---> H3O+(aq) + HCOO-(aq)

d)

NaOH(aq) --> Na+(aq) + OH-(aq)

e)

NH3(aq) + H2O(l) <---> NH4+(aq) + OH-(aq)

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