A student determines that an aqueous solution that contains 0.254 M sodium acetate and 0.417 M acetic acid, also has a H3O+ concentration of 3.90×10-5 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: CH3COOH(aq) + H2O --- H3O+(aq) + CH3COO-(aq) (1) as is usually done, without the inclusion of water in the expression for K:   K =  (2) for comparison, with the inclusion of water in the expression for K:   K =

Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2(aq) + H2O (l) <====> H3O+(aq) + NO2-(aq) In which direction will the equilibrium shift if NaOH is added?  NaNO2 is added ? HCl is added? The acid solution is made more dilute ?

Gypsum (CaSO4·2H2O) is added to soil to enhance plant growth. It dissolves according to the following equation: CaSO4⋅2H2O(s)⇌Ca2+(aq)+SO2−4(aq)+2H2O(1)CaSO4⋅2H2O(s)⇌Ca2+(aq)+SO42−(aq)+2H2O(1) The Ksp of gypsum is 3.14 × 10−5. How much gypsum, in grams, should you add to your 5.0 L watering can to produce a saturated solution?

You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth.  Y2O + Y2O  ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths place

The following reactions all have K > 1. 1) HC₂H704 (aq) + CIO (aq)C9H7O4 (aq) + HCIO (aq) 2) C6H5COOH (aq) + CIO (aq)HCIO (aq)+ CáH5COO* (aq) 3) HC₂H704 (aq) + C6H5COO (aq) = C9H704 (aq) + C6H5COOH (aq) Arrange the substances based on their relative base strength. C9H704 C6H5COO™ C6H5COOH HCIO Clear All strongest base intermediate base weakest base

7 8 9 6 Submit Tap here or pull up for additional resources 个 10 (aq) O H H₂O

A student determines that an aqueous solution that contains 0.173 M sodium hypochlorite and 0.391 M hypochlorous acid, also has a H3O* concentration of 1.11×10-7 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HCIO(aq) + H₂O=H3O*(aq) + CIO (aq) (1) as is usually done, without the inclusion of water in the expression for K: K= (2) for comparison, with the inclusion of water in the expression for K: K=

Write the equilibrium constant expression for this reaction: H₂SO4(aq) → 2H* (aq) + SO² (aq) x DO 8

Metal sulfides are prepared by bubbling hydrogen sulfide gas, H, S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H, S, which occurs when [H,S] = 0.100 M, the equilibrium shown is established. H, S(aq) + 2 H, O(1) = s²-(aq) + 2H,O*(aq) Keq = 1.1 x 10-20 An aqueous solution containing 0.0521 M Pb2+ and 0.0521 M Ag* is saturated with H, S. Above what concentration of S²- will PbS precipitate? The Kyp of PbS is 8.9 × 10-29. [s²-] = M Above what concentration of S²- will Ag,S precipitate? The Kşp of Ag,S is 3.3 × 10-50. [s²-] = M If the pH of the solution is adjusted to 2.32, which species will precipitate from the saturated H, S solution? both PbS and Ag,S PbS neither species O Ag,S

Given the two reactions 1. H2 S(aq) = HS (aq) + H†(aq), K1 = 9.15×10-8, and 2. HS (aq) = S²-(aq) + H+(aq), K2 = 1.39×10-19, what is the equilibrium constant Kfinal for the following reaction? s2- (аq) + 2H* (аq) = H2S(aq) Enter your answer numerically.