Calculate the solubility of AgCI(s) in water (Ksp = 1.6 times 10^-10) 1.6 times

Question

Calculate the solubility of AgCI(s) in water (Ksp = 1.6 times 10^-10) 1.6 times 10^-5 M 1.26 M 1.26 times 10^-5 M none of the above. The solubility of Fe(OH)_2 (Ksp = 1.6 times 10^-14) in water is 3.4 times 10^-4 M 8.0 times 10^-7 4.0 times 10^-4 M none of the above The solubility of a slightly soluble salt in the presence of a common ion increases decreases remains the same none of the above The ionization of a weak acid in the presence of a common ion increases decreases remains the same none of the above The ph of normal blood is greater than 7.0 less than 7.0 7.0 7.4 A buffer solution attempts to keep the pH of a solution constant upon addition of small concentration of acid small concentration of acid or base high concentration of acid or base B and C The pH of pure water is 7.4 7.0 less than 7.0 none of the above When the pH of blood is less than normal, a condition develops and it is known as acidosis alkalosis death blindness When the pH of blood is higher than normal, a condition develops and it is known as acid's alkalosis death blindness that is the reason for using buffer solutions in the laboratory? so as to keep the pH instant so as to get the desired product(s) so as to make the reaction go faster to reach equilibrium fast a strong acid and a weak electrolyte a strong acid and strong electrolyte C base and a weak electrolyte none of the above A has a pH of 5.9 while solution B has a pH of 12.9. Which solution is more acidic? solution A none of the above 0.350 M CH3COOH (Ka = 1.8 times 10^-5) aqueous solution [H^+] is 0.0089 M 2.5 times 10^-3 M HCI aqueous solution, [H^+] is 0.084 M 2.00 M 0.0089 M Ca(OH)_2aqueous solution, [H^+]is 0.005 M 0.01 M 0.0025 M of the solution in question # 13 is 2.72 2.60 0.350 none of the

Explanation / Answer

Agcl=Ag++Cl-

KSP=[Ag+][Cl-]

1.6*10-10=s*s

s=sqrt(1.6*10-10)

s=1.26*10^-5

Correct option is C

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