Consider the following reaction at equilibrium: Le Chatelier\'s principle predic

Question

Consider the following reaction at equilibrium: Le Chatelier's principle predicts that adding 0:(g) to the reaction container will decrease the partial pressure of CO_2(g) at equilibrium decrease the value of the equilibrium constant increase the partial pressure of CO_2(g) at equilibrium increase the partial pressure of CO(g) at equilibrium increase the value of the equilibrium constant What is the conjugate acid of HS-? H_3O+ H_2S S^2- OH- A solution with a hydroxide ion concentration of 4.15 times 10^-6 M is and has a hydrogen ion concentration of. Calculate the hydronium ion concentration in an aqueous solution with a pOH of 4.37 at 25degreeC. 7.1 times 10^-5 M 2.3 times 10^-10M 8.7 times 10^-10 m 6.5 times 10^-5 M 1.4 times 10^-10 M Determine the pH of a 0.850 M NH_4CI solution at 25degreeC. The K_b for NH_3 is 1.76 times 10^5. 2.73 4.66 5.27 7.45 9.52

Explanation / Answer

9.

adding a product, will favour production of reactants, that is, the shift goes toward left; more CO2 will be produced

10.

conjugate acid is H+ + HS- = H2S

11.

pH = -log(4.15*10^-6) = 5.381951

which is acidic since pH < 7

12.

pOH = 4.37

pH = 14-4.37

[H+] = 10^-pH = 10^-( 14-4.37) = 2.344*10^-10

13

this is a buffer pKb= 4.75 so

pOH = pKb = 4.75

14- 4.75 = 9.25

pH must be near 9.52

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