Please Help me with these problems! URGENT! What is the molar solubility of Ag2S
ID: 876555 • Letter: P
Question
Please Help me with these problems! URGENT!
What is the molar solubility of Ag2SO4 in 0.11 M Na2SO4? Ksp(Ag2SO4) = 1.5 ´ 10-5
A sample of hydrochloric acid (approximately 0.10 M) is titrated with 0.0993 M NaOH. What indicator changes color closest to the equivalence point?
In water, the solubility of Al(OH)3 is 1.08 ´ 10-4 M. Calculate Ksp.
What is the molar solubility of Ag2SO4 in the presence of 0.22 M aqueous solution of AgNO3? Ksp(Ag2SO4) = 1.5 ´ 10-5
What is the pH of a buffer solution that consists of 0.83 M HBrO and 0.53 M KBrO? Ka(HBrO) = 2.3 ´ 10-9
Consider titrating CH3COOH with standard NaOH (delivered from the burette) to answer the following question(s).
Refer to Exhibit 16-2. How would the pH be determined for the aqueous solution in the titration above at the equivalence point?
The molar solubility of SrF2 in water is 8.8 ´ 10-4 M. What is the solubility product constant, Ksp, for this substance?
Explanation / Answer
too many questions, let me try and put solutions for you.
1) Ksp = [Ag+]^2[SO4--]
1.5 x 10^-5 = [Ag+]^2[0.11]
[Ag+] = 0.0117 M or 0.0058 M [check which one is correct for you]
3) Ksp = [Ag+][OH-]^3
= (1.08 x 10^-4)(3.24 x 10^-4)^3
= 3.67 x 10^-15
4) Hendersen-Hasselbalck equation,
pH = pKa + log(salt/acid)
= 2.3 x 10^-9 + log(0.53/0.83)
= -0.195
5) In the titration of CH3COOH and NaOH, the pH above equivaence point is determined by first,
calculating the amount of OH- (since NaOH is in excess beyond equivalence point)
then find pOH
pH = 14 - pOH
6) Ksp = [Sr2+][F-]^2
= (8.8 x 10^-4)(1.76 x 10^-3)^2
= 2.8 x 10^-9