Question

Calculate the Ksp of Cd(OH)2 if 3.1 mL of 0.01300 M HCl was needed to titrate...

Calculate the Ksp of Cd(OH)2 if 3.1 mL of 0.01300 M HCl was needed to titrate 1.2 L of saturated Cd(OH)2 solution. (show your work)

Homework Answers

Answer #1

Number of moles of HCl, n = Molarity x volume in L

                                      = 0.01300 M x 3.1 mL x10-3 L/mL

                                     = 4.03x10-5 mol

2HCl + Cd(OH)2 ----> CdCl2 + 2H2O

From the balanced reaction ,

2 moles of HCl reacts with 1 mole of Cd(OH)2

4.03x10-5 moles of HCl reacts with ( 4.03x10-5 /2) = 2.015x10-5 moles of Cd(OH)2

So Molarity of Cd(OH)2 , M = Number of moles / volume in L

                                        = ( 2.015x10-5 mol) / 1.2 L

                                        = 1.68x10-5 M

Cd(OH)2 ----> Cd+ + 2 OH-

So [Cd2+] = [Cd(OH)2] = 1.68x10-5 M

[OH-] = 2x [Cd(OH)2] = 2x1.68x10-5 M = 3.36x10-5 M

Solubility product constant , Ksp = [Cd2+] [OH-]2

                                                = (1.68x10-5 )(3.36x10-5 )2

                                                = 1.89x10-14

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
0.02500 M EDTA solution were used to titrate 10.00 mL saturated Ca(OH)2 solution. EDTA=C10H14N2Na2O8 The average...
0.02500 M EDTA solution were used to titrate 10.00 mL saturated Ca(OH)2 solution. EDTA=C10H14N2Na2O8 The average volume of EDTA solution needed was 11.15 mL to titrate a 10.00 mL saturated solution of Ca(OH)2. milimoles of EDTA= 0.02500(M) *11.15ml = 0.2875milimoles Milimoles of Ca2+= strength * volume = 2.845milimoles ____________________________________________________________ 1.) How many grams of Ca(OH)2 can be dissolved in 1-L solution? 2.) Ksp
A 34.62 mL of 0.1510 M Ca(OH)2 was needed to neutralize 55.7 mL of an HCl...
A 34.62 mL of 0.1510 M Ca(OH)2 was needed to neutralize 55.7 mL of an HCl solution. What is the concentration of the original HC(aq) solution? please show work
I titrated a solution of 25.0 mL of a 0.050 M NaOH solution containing Ca(OH)2 using...
I titrated a solution of 25.0 mL of a 0.050 M NaOH solution containing Ca(OH)2 using 27.71 mL of standardized 0.065 M HCl. 1.) use the HCl volume and concentration to calculate [OH- ] in the saturated solution of Ca(OH)2 in NaOH solution. 2.) Using the known concentration of NaOH solution in Part B, calculate [OH- ] due to the NaOH alone. 3.) Calculate [OH- ] due to dissolved Ca(OH)2. 4.) Calculate [Ca^2+ ]. 5.) Calculate Ksp for Ca(OH)2 in...
For a saturated solution of an unknown metal hydroxide, M(OH)2 , 13.75 mL of this solutionwere...
For a saturated solution of an unknown metal hydroxide, M(OH)2 , 13.75 mL of this solutionwere required to neutralize 25.00 mL of 0.02 M HCl. Calculate the KSP of the metal hydroxide.
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The...
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The students found that 10.10-mL of acid was required to reach the equivalence point. Calculate the molar concentration of OH- and Ca2+, the molar solubility, and Ksp of the analyte. Show detailed calculation for each. [OH-] in the analyte: [Ca2+] in the analyte: molar solubility of Ca(OH)2: Ksp of Ca(OH)2:
0.050 M HCl Volume at equivalence point = 10.37 mL Volume of Ca(OH)2 used in the...
0.050 M HCl Volume at equivalence point = 10.37 mL Volume of Ca(OH)2 used in the titraiton = 15 mL a) What happens at equivalence point? b) Calculate the [OH-]. c) Calculate the [Ca+2]. d) Calculate the Ksp for Ca(OH)2. e) What is the concentration (in molarity) of the saturated Ca(OH)2?
1) Calculate the solubility of manganese(II) hydroxide, Mn(OH)2 in units of grams per liter. Ksp(Mn(OH)2) =...
1) Calculate the solubility of manganese(II) hydroxide, Mn(OH)2 in units of grams per liter. Ksp(Mn(OH)2) = 4.6×10-14. solubility = ? g/L 2)The equilibrium concentration of hydroxide ion in a saturated lead hydroxide solution is ? M. 3) The mass of aluminum phosphate that is dissolved in 225 mL of a saturated solution is ? grams.
Will a precipitate form if 100.0 mL of 2.5 x 10-3 M Cd(NO3)2 and 75.0 mL...
Will a precipitate form if 100.0 mL of 2.5 x 10-3 M Cd(NO3)2 and 75.0 mL of 0.0500 M NaOH are mixed at 25o C? (Yes or No) Calculate the concentration of cadmiun ion in solution at equilibrium after the two solutions are mixed. (Ksp is 7.2 x 10-15 for Cd(OH)2 at 25o C) Please show all work.
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL)...
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL) = 25.0 mL 2. Concentration of Standardized HCL solution (mol/L) = 0.05 mol/L 3. Buret reading, initial (mL) = 50.0 mL 4. Buret reading, final (mL) = 32.5 mL 5. Volume of HCL added (mL) = 17.5 mL 6. Moles of HCL added (mol) = (concentration of HCl)(Volume of HCl) = (0.05)(19.1) = 0.875 mol. 7.Moles of OH- in saturated solution (mol)=8.75x10^-4 8.the [OH-]...
How many grams of Pb(OH)2 will dissolve in 500 mL of a 0.050-M PbCl2 solution? Ksp...
How many grams of Pb(OH)2 will dissolve in 500 mL of a 0.050-M PbCl2 solution? Ksp =1.2 x10^-5