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1.The observed solubility of the salt MX in 4.0?M?strong acid is 2.30 x?10?3?M.? The?Ka?value for the acid HX is 1.00 x?10?9.? Calculate the value of?Ksp?for the salt MX.

2.Consider a solution made by mixing 500.0 mL of 4.0?M?NH3?and 500.0 mL of 0.40?M?AgNO3. Ag+?reacts with NH3?to form AgNH3+?and Ag(NH3)2+:

 Ag+?+ NH3??AgNH3+ K1?= 2.1 x?103 AgNH3+?+ NH3??Ag(NH3)2+ K2?= 8.2 x?103

The concentration of Ag(NH3)2+?at equilibrium is____?

3.Given the following values of equilibrium constants:

 Cu(OH)2(s)??Cu2+(aq) + 2OH?(aq) Ksp?= 1.6 x?19?19 Cu(NH3)42+(aq)??Cu2+(aq) + 4NH3(aq) K?= 1.0 x?10?13

What is the value of the equilibrium constant for the following reaction?
????????? Cu(OH)2(s) + 4NH3(aq)??-->Cu(NH3)42+(aq) + 2OH?(aq)

4.Calculate the molar concentration of uncomplexed Zn2+?in a solution that contains 0.20 mol of Zn(NH3)42+per liter. The overall?Kf?for Zn(NH3)42+?is 3.8 x?109.

5.

A 50.0-mL sample of 2.0 x?10?4?M?CuNO3?is added to 50.0 mL of 4.0?M?NaCN. Cu+?reacts with CN??to form the complex ion Cu(CN)32?:

 Cu(CN)32???Cu+?+ 3CN? K?= 1.0 x?10?9

Calculate the solubility of CuBr(s) (Ksp?= 1.0 x?10?5) in 1.0 L of 1.0?M?NaCN.

1.? A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.11 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 x 10^-5)

2.?After adding 25.0 mL of 0.100?M?NaOH to 100.0 mL of 0.100?M?weak acid (HA), the pH is found to be 5.90.? Determine the value of?Ka?for the acid HA.

3.For carbonic acid (H2CO3),?Ka1?= 4.30 x?10?7?and?Ka2?= 5.62 x?10?11. Calculate the pH of a 0.50?M?solution of Na2CO3.

1.? A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.11 M NH3. What is the resulting pH? (Kb for NH3 = 1.8 x 10^-5)

2.?After adding 25.0 mL of 0.100?M?NaOH to 100.0 mL of 0.100?M?weak acid (HA), the pH is found to be 5.90.? Determine the value of?Ka?for the acid HA.

3.For carbonic acid (H2CO3),?Ka1?= 4.30 x?10?7?and?Ka2?= 5.62 x?10?11. Calculate the pH of a 0.50?M?solution of Na2CO3.

4.Calculate the pH when 200.0 mL of a 1.00M?solution of H2A (Ka1= 1.0 x?10?6,?Ka2= 1.0 x?10?10) is titrated with the following volumes of 1.00MNaOH.

150.0 mL of 1.00MNaOH

5.Consider the titration of 200.0 mL of a 0.100?M?solution of the weak acid H2A with 0.200?M?NaOH.? The first equivalence point is reached after 100.0 mL of 0.200?M?NaOH has been added, and the pH is 6.27.? The pH, after 65.0 mL of 0.200?M?NaOH has been added, is 4.95.

Calculate the value of?Ka1?for H2A.

Thank you!!

4.Calculate the pH when 200.0 mL of a 1.00M?solution of H2A (Ka1= 1.0 x?10?6,?Ka2= 1.0 x?10?10) is titrated with the following volumes of 1.00MNaOH.

150.0 mL of 1.00MNaOH

5.Consider the titration of 200.0 mL of a 0.100?M?solution of the weak acid H2A with 0.200?M?NaOH.? The first equivalence point is reached after 100.0 mL of 0.200?M?NaOH has been added, and the pH is 6.27.? The pH, after 65.0 mL of 0.200?M?NaOH has been added, is 4.95.

Calculate the value of?Ka1?for H2A.

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