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13&14 please! Question 13 Write the equilibrium expression for the following reaction. HCIO4 (aq) -> H+...
Calculate the OH- concentration at equilibrium in the following reaction: NH3 (aq) + H20 (1) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5) (1 point) O 1x10^(-14) M O2.7 x10^(-3) M O 7.2 x10^(-6) M O None of the above Question 15 Which of the following pH values indicates the most basic solution? (1 point)* O pH=12 O pH=4 O pH=8 O pH=9
Question 10 Which of the following IS a strong acid (1 point ) * H2SO4 HCN HF NH3 Question 11 Write the equilibrium expression for a simple acid ionization. (HA (aq) -> H+ + A-) (1 point ) * Ka = ([H+][A-])/[HA] Ka = [H+]/[HA] Ka = [H+][A-] None of the above Question 12 Write the equilibrium expression for the following reaction. HF (aq) -> H+ (aq) + F- (aq) (1 point ) * Ka = ([H+][F-])/[HA] Ka = [H+]/[HA]...
1) Calculate the OH- concentration at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5). (a) 1 x10^(-14) M (b) 2.7 x10^(-3) M (c) 7.2 x10^(-6) M (d) None of the above 2) Which of the following pH values indicates the most basic solution? (a) pH=12 (b) pH=4 (c) pH=8 (d) pH=9 3) Which of the following pH values indicate the most acidic solution? ( (a) pH=11 (b) pH=2...
Calculate the concentration of OH- at equilibrium in the following reaction: NH3 (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) (Kb = 1.8 x10^(-5)
11&12 please! Question 11 Write the equilibrium expression for a simple acid ionization. (HA (aq) -> H+ + A-) (1 point) * Ka = ([H+][A-])/[HA] O Ka = [H +)/(HA) Ka = [H +][A-] O None of the above Question 12 Write the equilibrium expression for the following reaction. HF (aq) -> H+ (aq) + F- (aq) (1 point) * O Ka = ([H+][F-1)/(HA) O ka = [H +)/(HA) Ka = [H +][F-1 O None of the above
For aq. solutions of salt NH4NO2, following reactions possible: NH4+ + NO2- -> NH3 + HNO2 k1? NH4+ + H2O -> H3O+ + NH3. ka = 5.6 x 10^-10 NO2- + H2O -> HNO2 + OH- kb =2.2 x 10^-11 2H2O -> H3O+ + OH- kw = 1.0 x10^-14 Write symbolic expression for equilibrium constants for each reaction. Derive expression for k1 in terms of ka, kb, and kw; find numerical value of k1.
For the reaction NH3(aq) + H+ (aq) ⇋ NH4 + (aq), at 20°C the equilibrium concentrations were as follows: [NH3] = 2 x 10-4 M; [H+ ] = 2 x 10-4 M; and [NH4 + ] = 18 M. Calculate the equilibrium constant for the reaction.
3&4 please! Question 3 Based on the ion-product constant (Kw), calculate the concentration of H+ ions if the concentration of OH-ions is 2 x10^(-7) M. (1 point)* O 1x10^(-14) M O 2x10^(7) M 5 x10^(-8) M None of the above Question 4 Calculate the pH of a solution if the concentration of H+ is 2.67 x10^(-5) M (1 point) * O 11 4.57 O 7 None of the above
7&8 please! Question 7 Calculate the pH of a solution if the concentration of OH-is 6.79 x10^(-8) M (1 point) O 14 O 6.83 O 7.17 O None of the above Question 8 Calculate the concentration of H+ ions if the pOH of the solution is 3.56. (1 point) O 1x10^(-14) M O 2.75 x10^(-4) M O 3.63 x10^(-11) M O None of the above
Calculate the equilibrium concentrations of all chemical species present in a 0.10 M H CO.(aq) solution. What is the percent ionization of the acid and resulting pH? Units Units [H2CO3) = Number [HCO3) = Number [CO32) = Number [H30+) = Number Units Units % ionization = Number pH = Number Ka Acid Acetic Ammonium Formula CH3COOH NH4+ H3B03 1.8 x 10-5 5.6 x 10-10 5.4 x 10-10 Boric Carbonic H2CO3 Chlorous Formic Hydrocyanic Perchloric HCIO2 HCOOH HCN HC104 4.5 x...