6.
a.
b.
c.
Since fluoride ions are removed (by reaction with calcium ions to form calcium fluoride), the equilibrium for dissociation of HF will shift to right. More and more HF will dissociate to produce more and more protons and fluoride ions. This will compensate for removal of fluoride ions (through reaction with calcium ions). Due to this, the concentration of HF will decrease and the concentration of protons will increases.
d.
Added NaF is strong electrolyte and completely dissociates to provide fluoride ions (common ions). This will increase fluoride ion concentration. Due to this, the equilibrium for dissociation of HF will shift to left. More and more protons will combine with fluride ions to provide HF. Due to this fluoride ion concentration will decrease. This will compensate for added fluoride ions (in the form of NaF). Due to this, concentration of HF will increase and that of protons will decrease. This illustrates common ion effect.
e.
Since the temperature is same, the value of the equilibrium constant is also same.
f.
Endothermic reaction means heat is supplied during reaction.
With increase in temperature, heat is supplied to the reaction mixture. Here heat appears on reactant side. Due to this, the equilibrium for dissociation of HF will shift to right. More and more HF will dissociate to produce more and more protons and fluoride ions. The concentration of HF will decrease and the concentration of protons will increases.
question 6 a-f 6. The dissociation reaction for hydrofluoric acid is shown below. HF (aq) =...
Below is a diagram illustrating a mixture HF and Fin 161 16 an aq solution. For this mixture, does pH equal pK, for HF? Describe how the number of HF molecules and F ions incre nge after three OH ions are added. How will the num- cati ofHF and F change if two H ions are added? Explain your dare easte will change ber o answers by using chemical equations Explain your dres 16. Pro pr 16 or
Consider the buffer system of hydrofluoric acid. HF. and its salt. NaF. HF(aq) + H2O() E H 0*(aq) + F(aq) a. The purpose of this buffer system is to: 1. maintain (HF] 2. maintain [F] 3 maintain pH b. The salt of the weak acid is needed to: (1) provide the conjugate base 2. neutralize added 1,0 3. provide the conjugate acid c. If OH is added, it is neutralized by: 1. the salt 2. HO 3. H,00
2. HF ionizes in water to produce H.O'(aq) and F (aq) ions. 0.22 M Naf solution is added to a 0.10 M HF(aq) at 25°C. The Ka of HF is 3.5 x 10-5. (Hint: NaF is a salt. F is the common ion for the equilibrium). Calculate the pH of the solution. Show work.
ben 39. Write the expression for K for the reaction of hydrofluoric acid with water. HF(aq)+ H2O()F (aq)+ H50 (aq) stes boda a. b i boooong or oto bodedao bsde ey to ednbo od is K = hddp lin stondinpo fan Ersd ealoinen b. K = - [H,0"] o cmuloy sdt oab sob eno С. F K [HF] d. K = [HF] [HF] e. K = [FE,0"]
HF(aq) reacts with NaOH(aq) according to the reaction represented below. HF(aq) + OH(aq) - H2O(l) + F(aq), K-7.2x 10-4 A volume of 15 mL of 0.40 M NaOH(aq) is added to 25 mL of 0.25 M HF(aq) solution. Assume that volumes are additive. Write up to 8 correct, distinct and relevant facts about this reaction and any other information given. You'll earn 1 point for each correct statement. Five statements will get you full credit. Only the first eight statements...
Write the concentration equilibrium constant expression for this reaction. HF(aq)+H2O(1-F (aq)-H,0 (aq)
estion 10 of 65 > Consider the reaction. HF(aq) + KOH(aq) — KF(aq) + H20(1) What is the net ionic equation for the chemical reaction? HF(aq) + K+(aq) + OH(aq) — K+(aq) + F (aq) + H2O(1) O HF(aq) + K+(aq) + OH-(aq) — K+(aq) + F (aq) + H+(1) + OH-(1) O HF(aq) + OH-(aq) —> F-(aq) + H2O(1) HF(aq) + K+(aq) F (aq) + H+(1) HF(aq) + K+(aq) K+(aq) + H2O(1) - 11 of 65 > Calculate either...
Write the concentration equilibrium constant expression for this reaction. F (aq)+H,0" (aq)HF (aq)+H20(1) dº do * $ ?
FeF2(s) = Fe2+(aq) + 2 F"(aq) F(aq) + H*(aq) = HF(aq) FeF2(s) + 2 H+ (aq) = Fe2+ (aq) + 2 HF(aq) K1 = 2 x 10-6 K2 = 1 x 103 K3 = ? Decide whether the last reaction is thermodynamically favorable. Justify your answer.
Use this description to answer the questions: Solution 1 is 0.1M weak acid HF and the pH is found to be 2.8. Write the acid dissocation reaction for HF. Solution 2 consists of the same 0.1 M weak acid HF but in 1.0M sodium nitrate. Write T if the statement is true, F if it is false. The pH of solution 1 and solution 2 will be the same within statistical error. The pH of solution 2 will be lower...