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16 Nov 2019
Suppose a buffer solution is made from formic acid, HCHO_2, and sodium formate, NaCHO_2. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? a) NaoH (aq) + H_3O^+ (aq) rightarrow Na^+ (aq) + 2H_2O(l) b. H_3O^+ (aq) + OH^- (aq) rightarrow 2H_2O(l) c) OH^- (aq) + HCHO_2(aq) rightarrow CHO_2^- (aq) + H_2O(l) d) NaOH(aq) + HCHO_2(aq) rightarrow NaCHO_2(aq) + H_2O(l) e) NA^+ (aq) + HCHO_2(aq) rightarrow NaH(aq) + HCO_2^+(aq) A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCL is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing? a) OH^- b) Na^+ c) F^- d) Na^- e) none of these The following question refers to the following system: A 1.0-liter solution contains 0.25 M HF and 0.66 M NaF (K_a for HF is 7.2 times 10^-4). If one adds 0.30 liters of 0.020 M KOH to the solution, what will be the change in pH? a) 0.01 b) 3.58 c) 0.44 d) -0.09 e) -0.22
Suppose a buffer solution is made from formic acid, HCHO_2, and sodium formate, NaCHO_2. What is the net ionic equation for the reaction that occurs when a small amount of sodium hydroxide is added to the buffer? a) NaoH (aq) + H_3O^+ (aq) rightarrow Na^+ (aq) + 2H_2O(l) b. H_3O^+ (aq) + OH^- (aq) rightarrow 2H_2O(l) c) OH^- (aq) + HCHO_2(aq) rightarrow CHO_2^- (aq) + H_2O(l) d) NaOH(aq) + HCHO_2(aq) rightarrow NaCHO_2(aq) + H_2O(l) e) NA^+ (aq) + HCHO_2(aq) rightarrow NaH(aq) + HCO_2^+(aq) A weak acid, HF, is in solution with dissolved sodium fluoride, NaF. If HCL is added, which ion will react with the extra hydrogen ions from the HCl to keep the pH from changing? a) OH^- b) Na^+ c) F^- d) Na^- e) none of these The following question refers to the following system: A 1.0-liter solution contains 0.25 M HF and 0.66 M NaF (K_a for HF is 7.2 times 10^-4). If one adds 0.30 liters of 0.020 M KOH to the solution, what will be the change in pH? a) 0.01 b) 3.58 c) 0.44 d) -0.09 e) -0.22
Trinidad TremblayLv2
1 Apr 2019