Question

What is the solubility in moles/liter for silver bromide at 25 oC given a Ksp value...

What is the solubility in moles/liter for silver bromide at 25 oC given a Ksp value of 7.7 x 10-13. Write using scientific notation and use 1 or 2 decimal places (even though this is strictly incorrect!

Homework Answers

Answer #1

Ksp of AgBr = 7.7 x 10^-13

AgBr   --------------> Ag+   +     Br-

                                  S             S

Ksp = S^2

7.7 x 10^-13 = S^2

S = 8.77 x 10^-7 M

molar solubility = 8.77 x 10^-7 M

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1)At 25 oC the solubility of silver iodide is 8.94 x 10-9 mol/L. Calculate the value...
1)At 25 oC the solubility of silver iodide is 8.94 x 10-9 mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect) 2)The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of Al(OH)3 in 0.0000010 M Al(NO3)3? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).
What is the solubility in moles/liter for calcium sulfate at 25 oC given a Ksp value...
What is the solubility in moles/liter for calcium sulfate at 25 oC given a Ksp value of 2.4 x 10-5
1. At 25 oC the solubility of lead(II) iodide is 1.52 x 10-3 mol/L. Calculate the...
1. At 25 oC the solubility of lead(II) iodide is 1.52 x 10-3 mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect). 2. At 25 oC the solubility of zinc hydroxide is 1.71 x 10-6 mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect).
The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of Al(OH)3 in a...
The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of Al(OH)3 in a solution that has a pH =13? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).
Calculate the Ksp (solubility product CONSTANT) value of AgI if at equilibrium [I -] = 1.23...
Calculate the Ksp (solubility product CONSTANT) value of AgI if at equilibrium [I -] = 1.23 x 10 -6 M (Hint: write the balanced chemical reaction and Ksp expression) Enter using 'e' notation: .00555 would be entered 5.55e-3
Gold(III) chloride, AuCl3, has Ksp= 3.2 x 10-25. Calculate the molar solubility of gold(III) chloride in...
Gold(III) chloride, AuCl3, has Ksp= 3.2 x 10-25. Calculate the molar solubility of gold(III) chloride in pure water and in various aqueous solutions. Put your answers with 2 significant figures. Calculate the molar solubility of gold(III) chloride in 0.010 M Au(NO3)3 solution. Enter your response in scientific notation, e.g. enter 2E3 for 2000
What is the value of ΔGo in kJ at 25 oC for the reaction between the...
What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: Br2(l) and Cl-(aq) Use the reduction potential values for Br2(l) of +1.07 V and for Cl2(g) of +1.36 V Give your answer using E-notation with ONE decimal place (e.g., 2.1 x 10-2 would be 2.1E-2; and 2.12 x 10-2 would also be 2.1E-2.).
A)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2...
A)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2 in pure H2O ? 2.41×10−4 M B)Based on the given value of the Ksp , what is the molar solubility of Mg(OH)2 in 0.200 M NaOH ? Ksp , of 5.61×10−11 D) What is the pH change of a 0.300 M solution of citric acid (pKa=4.77 ) if citrate is added to a concentration of 0.140 M with no change in volume?
(A) Using the Ksp for Cu(OH)2 (1.6 x 10^-19) and the overall formation constant for Cu(NH3)4...
(A) Using the Ksp for Cu(OH)2 (1.6 x 10^-19) and the overall formation constant for Cu(NH3)4 (1.0 x 10^13), calculate a value for the equilibrium constant for the reaction: Cu(OH)2(s) + 4NH3(aq) <===> Cu(NH3)4(aq) + 2OH-(aq) (B) Use the value of the equilibrium constant you calculated in Part A to calculate the (approximate) solubility (in mols/liter, M) of Cu(OH)2 in 5.0 M NH3. In 5.0 M NH3 the concentration of OH- is 9.5 x 10^-3 M. (Although not strictly correct...
Part I A) The solubility of silver bromide can be increased by dissolving it in a...
Part I A) The solubility of silver bromide can be increased by dissolving it in a solution containing the thiosulfate anion. AgBr(s) Ag+ (aq) + Br- (aq)    K1 = 7.7 x 10-13 Ag+(aq) + 2S2O32- (aq) Ag(S2O3)23- (aq)     K2 = 4.7 x 1013 What is the value of the equilibrium constant for the overall reaction? AgBr(s) + 2S2O32-(aq) Ag(S2O3)23-(aq) + Br-(aq)    a) 12.4x1013 b) 3.6x10-9    c) 4.7x10-9   d) 4.7x1013    e) 36 B) Consider the following reaction at...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT