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Which of the following salts gives the following Ksp expression?
Ksp=27s4
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- For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?What will happen if the pH of the following equilibrium system is increased? H*(aq) + 2CrO4²a yellow The solution will turn yellow. b. The solution will turn a darker orange. There will be no effect on the equilibrium system. 2- aq) O Cr20,² (aq) + OH (аq) orange а. с. d. The concentration of OH will decrease. (aq) All hydroxide ion will be used up. е.57. Consider the reaction: MISSED THIS? Read Section 16.8; Watch KCV 16.8, IWE 16.12 HC,H,O;(aq) + H,0(1) = H;O*(aq) + C,H;O, (aq) K = 1.8 x 10 $ at 25 °C If a solution initially contains 0.210 MHC,H;02, what is the equilibrium concentration of H,0*at 25 °C?
- 2. In the following reaction at equilibrium: 2CrO,? (aq, yellow) + 2 H;O* (aq) =Cr2O;?- (aq, orange) + 3 H20 (1) A. What color change do you observe when you add NaOH? B. How is this observation consistent with Le Chatlier's principle? Write the chemical equation that accounts for the change and briefly explain.4. A solution at 25°C is prepared in which a very small amount of Fe2+ is added to a much larger amount of solution in which the [OH-] is 1.0 x 10-2M. Some Fe(OH)2 precipitates. The value of Ksp for Fe(OH)2 = 8.0 x 10-10. a. Assuming that the [OH-] = 1.0 x 10-2M, calculate the [Fe2+].Phosphoric acid dissociates to form phosphate anion and hydronium cation. The K, for this reaction is 4.5 x 10-13. Choose the corre equation which expresses this reaction. 4.5 x 10 13 = ([PO4°] x [H3O*j³ ) / ( [H3PO4] × [H2O] ) 4.5 x 10 13 = ([PO4°] × [H3O*] ) / [H3PO4] 4.5 x 1013 = ( [PO4³] × [H3O*]³ ) / [H3PO4] %3D 4.5 x 10 13 = [H3PO4] / ( [PO43-] × [H3O*j³ ) %3D 5 Question 14
- There is a solution containing 5M of PO43- at room temperature. Using the following Ka values, find the equilibrium concentration of PO43-, HPO42-, H2PO4-, H3PO4 and OH--10 a. Obtain the K value for CN. Ka for HCN is 4.9 × 10 K, b. Obtain the Ka value for NH3 OH. K, for NH2OH is 1.1 x 10-8 KoAt 25°C, K = 3.40 x 10-3 S m-1 for 0.00100 M NH4OH. Values of Lo are: NH4C1 = 0.01497, NaOH = 0.02481, NaCl = 0.01265 S m2 mol-1. Find the dissociation constant of ammonium hydroxide.
- What is the K, reaction of HCN? K, reaction: The K, of HCN is 6.2 x 10-10. What is the Kb value for CN at 25 °C? KbIf H+ ion is added to a reaction where: AgC2H3O2(s) + Cl-(aq) becomes AgCl(s) + C2H3O2-(aq), would more AgCl precipate? I am not sure if H+ ion would react with Cl- ion in the reaction. Calculated K for the reaction above is 1.1 times 107.If 13.0 mL of 0.19 M MgCl2 are mixed with 21.9 mL of 0.54 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 ✕ 10-11 for Mg(OH)2. (in M)
