Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.
Part A
MX ( K sp = 5.30×10−11)
Express your answer in moles per liter.
Part B
Ag2CrO4 (Ksp = 1.12×10−12)
Express your answer in moles per liter.
Part C
Ni(OH)2 (Ksp = 5.48×10−16)
Express your answer in moles per liter.
A)
At equilibrium:
MX
<---->
M+
+
X-
s
s
Ksp = [M+][X-]
5.3*10^-11=(s)*(s)
5.3*10^-11= 1(s)^2
s = 7.28*10^-6 M
Answer: 7.28*10^-6 M
B)
At equilibrium:
Ag2CrO4 <----> 2
Ag+
+ CrO42-
2s
s
Ksp = [Ag+]^2[CrO42-]
1.12*10^-12=(2s)^2*(s)
1.12*10^-12= 4(s)^3
s = 6.542*10^-5 M
Answer: 6.54*10^-5 M
C)
At equilibrium:
Ni(OH)2 <---->
Ni2+
+ 2
OH-
s
2s
Ksp = [Ni2+][OH-]^2
5.48*10^-16=(s)*(2s)^2
5.48*10^-16= 4(s)^3
s = 5.155*10^-6 M
Answer: 5.16*10^-6 M
Use the Ksp values to calculate the molar solubility of each of the following compounds in...
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. You may want to reference (Pages 739 - 745) section 18.5 while completing this problem. Part A MX (Ksp = 8.53x10-11) Express your answer in moles per liter. V AE R O ? Submit Request Answer Part B Ag, CrO4 (Ksp = 1.12x10-12, Express your answer in moles per liter. 190 ADP * O O ? Submit Request Answer Part C Ni(OH)2...
II Review | Constants | Periodic Table Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. Part A You may want to reference (Pages 769 - 775) Section 17.5 while completing this problem. MX (Ksp = 2.37x10-36) Express your answer in moles per liter. EVO AQ R o 2 ? S = M Submit Request Answer Part B PbCl2 (Ksp = 1.17x10-5) Express your answer in moles per liter. V ALO...
A 0.5240 −g sample of an unknown monoprotic acid was titrated with 9.94×10−2 M NaOH. The equivalence point of the titration occurs at 23.90 mL . Determine the molar mass of the unknown acid. Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. PART A---- MX (Ksp = 8.57×10−36)Express your answer in moles per liter. PART B----PbCl2 (Ksp = 1.17×10−5) Express your answer in moles per liter. PART C-----Ni(OH)2 (Ksp =...
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. MX (Ksp = 5.35
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. MX (Ksp = 1.36×10−38) Update:thats all i was given for the qs. i guess it be an akali metal halide (MX).
(Post-Lecture Ch 17 Exercise 17.86 - Enhanced - with Feedback Part B Use the K, values to calculate the molar solubility of each of the following compounds in pure water You may want to reference (Pages 769 - 775) Section 175 while completing this problem Ag, CO, (K. = 1.12x10-12) Express your answer in moles per liter. V AED 1.03. 10-4 Submit Previous Answers Request Answer * Incorrect; Try Again Part C Ca(OH), (K. = 4.68x10-6) Express your answer in...
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...
Calculate the molar solubility of compounds in the following conditions: a. MgCO3 (Ksp = 3.49 x 10-8) in a solution containing 0.175 M Na2CO3? b. BaF2 (Ksp = 1.01 x 10-6) in a solution containing 0.125 M KF? c. Ag2CrO4 (Ksp = 1.12 x 10-12) in a solution containing 0.450 M Na2CrO4? d. Cu3(AsO4)2 (Ksp = 7.57 x 10-36) in a solution containing 0.325 M CuCl2? e. Ca3(PO4)2 (Ksp = 1.99 x 10-29) in a solution containing 0.325 M K3PO4?
Which compounds listed below has the smallest molar solubility in water and which compound has the highest molar solubility in water? (a) AgBr, Ksp = 5.35 x 10-13 (b) CaCO3, Ksp = 4.96 x 10-9 (c) Ag2CrO4, Ksp = 1.12 x 10-12 (d) CaF2, Ksp = 1.46 x 10-10 (e) CrF3, Ksp = 6.60 x 10-11
ksp = 5.48 x 10^-16 - ADVANCED MATERIAL Calculating the solubility of an lonic compound when a common ion is present Calculate the solubility at 25 C of NI(OH), in pure water and in a 0.0160 M NaOH solution. You'll find K. data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0160 M NaOH solution: 0 x 5 ?