A solution containing a mixture of 0.0441 M 0.0441 M potassium chromate ( K 2 CrO 4 K2CrO4 ) and 0.0513 M 0.0513 M sodium oxalate ( Na 2 C 2 O 4 Na2C2O4 ) was titrated with a solution of barium chloride ( BaCl 2 BaCl2 ) for the purpose of separating CrO 2− 4 CrO42− and C 2 O 2− 4 C2O42− by precipitation with the Ba 2+ Ba2+ cation. The solubility product constants ( ? sp Ksp ) for BaCrO 4 BaCrO4 and BaC 2 O 4 BaC2O4 are 2.10× 10 −10 2.10×10−10 and 1.30× 10 −6 1.30×10−6 , respectively. Which barium salt will precipitate first? BaC 2 O 4 BaC2O4 BaCrO 4 BaCrO4 What concentration of Ba 2+ Ba2+ must be present for BaCrO 4 BaCrO4 to begin precipitating? [ Ba 2+ ]= [Ba2+]= M M What concentration of Ba 2+ Ba2+ is required to reduce the oxalate ion to 10% 10% of its original concentration? [ Ba 2+ ]= [Ba2+]= M M What is the ratio of oxalate to chromate when the Ba 2+ Ba2+ concentration is 0.0060 M 0.0060 M ? [ C 2 O 2− 4 ] [ CrO 2− 4 ] = [C2O42−][CrO42−]=
A solution containing a mixture of 0.0441 M 0.0441 M potassium chromate ( K 2 CrO...
Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4and BaCrO4are 1.1 × 10^-12 and1.2 ×10^-10, respectively. ANSWER SAYS 3.2 x 10^-4 M Can someone explain how they got the answer? (3.2 x 10^-4 M)
Calculate the concentration in M) of barium ions (Ba2+) in a solution when BaCrO4 is dissolved in a solution that already contains 0.085 M of Cro 2-. The Ksy of BaCrO4 is 2.1 x 10-10 (4 points)
Calcium phosphate (Ca3(PO4)2) is sparingly soluble in water. If the concentration of calcium ions in solution at equilibrium is 1.0 x 10°M, what is the Ksp of calcium phosphate? a. 4.4 x 10-46 b. 2.2 x 10-46 c. 1.1 x 10-46 d.5.5 x 10-47 a. b. O C. d. KESCION 20 5 pts 14a) Sodium chromate is added to a solution of 0.0060 M 5r2+ What is Q if the final concentration of Cro 2 is 0.0030 M? a. 7.2...
A solution contains 1.30×10-2 M silver nitrate and 6.43×10-3 M calcium acetate. Solid potassium chromate is added slowly to this mixture. What is the concentration of silver ion when calcium ion begins to precipitate? [Ag+] = M
A solution contains 1.09x10-2 M calcium nitrate and 8.55x10-3 M lead acetate. Solid ammonium chromate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula B. What is the concentration of chromate ion when this precipitation first begins? [Cro_2-1- M Solubility Product Constants (Ksp at 25 °C) Type Ksp Formula ZnCO3 1.5 x 10-11 Chlorides PbCl2 1.7 x 10-5 AgCi 1.8 10-10 Chromates BaCrO4 2.0 10-10 CaCrO4 7.1 x 10-4 PbCr04 1.8...
28) What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 11.18? Ksp for Mg(OH)2 is 5.6x 10-12 B) 5.6x 10-10 M D) 1.1 x 10-4 M C) 2.4 x 10-6 M A) 5.6 x 10-8 M 29) What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 x 10-10 and Kf for Ag(CN) 2- is 1.0 x 1021, D) 0.050...
LABORATORY REPORT FORM 1. Molarity thiosulfate solution 0.01119 M 25°C 40°C 2. Actual solution temperature 25 40 c 3. Volume of sample withdrawn 20.00 20.00 20.00 20.00 mL 4. Initial buret reading 0.30 0.25 0.05 0.49 mL 5. Final buret reading 22.10 22:40 28.90 26.25mL 6. Volume thiosulfate used 21.80 22.15 28.85 25.76 mL 7. Volume thiosulfate used in liters 0.02 180 0.0.2215 0.02885 0.02574 8. Moles of thiosulfate used 2.44X10-49 48*104 8-234104288xthole 2.439x1074 2.479x104 3.228*10*4 2.882X10-9 9. Moles of...
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
1. 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 6.0 x 10-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x 10-5 and 1.8 x 10-10] 2. Which of the following is the expression for the solubility product of Ba3(AsO4)2? 3. The pKa of a weak acid is 6.50. What...
Question 21 8 pts A solution has a OH-concentration [OH-] = 2.5 x 10-4 M. a. Calculate the hydronium ion [H3O+] concentration in molarity. (Show all your work !!!!!) b. Calculate the pH and tell whether the solution is acidic or basic. (Show all your work !!!!!) 12pt v Paragraph v BI U A Av Tev : Question 20 6 pts Given the following chemical reaction, determine how many moles of HNO3 are reacted to make 22.7 g of H20....