Question 2 2 pts Solid Mn(OH)2 is added to a solution of 0.100 M FeCl2 What...
write the specific defenintion on Ksp found in your text boo Question 3 2 pts Solid Mn(OH)2 is added to a solution of 0.100 M FeCl2. After reaction, what will be the molar concentration of Fe2+ ? Helpful formulas: Mn(OH)2(s) 6Mn2+ (aq) + 2OH (aq) Ksp = 1.6 x 10-13 FeCl2(s) Fe2+ (aq) + 2OH- (aq) Ksp = 4.9 x 10-17 O 1.1 x 10-1 M. O 6.8 x 10-2 M. O 0.07 M. O 0.100 M
Question 18 3 pts What [NH4Cl] must be added to a solution of 273 M NH3(aq) to make a buffer of pH 9.402 O 1.82M 0.235 M O 5.17 M 0.386M 0.191M If poH = 8.8, what is [н']? pH рон [н'] [ОН ) 8.8 ? 1.6x 10:9 м o 5.5x 10:3М O 1.6x 105 м o 6.3x 10:6 м o 5.2 м
What would the solubility of [Pb(OH)3]-(aq) be in 0.100 M Ba(OH)2 in the presence of excess Pb(OH)2(s)? Ksp Ba(OH)2 = 5.0 x 10-3 Ksp Pb(OH)2 = 1.43 x 10-20 Kf [Pb(OH)3]- = 3.8 x 1014
What would the solubility of [Pb(OH)3]-(aq) be in 0.100 M Ba(OH)2 in the presence of excess Pb(OH)2(s)? Ksp Ba(OH)2 = 5.0 x 10-3 Ksp Pb(OH)2 = 1.43 x 10-20 Kf [Pb(OH)3]- = 3.8 x 1014
What would the solubility of [Pb(OH)3]-(aq) be in 0.100 M Ba(OH)2 in the presence of excess Pb(OH)2(s)? Ksp Ba(OH)2 = 5.0 x 10-3 Ksp Pb(OH)2 = 1.43 x 10-20 Kf [Pb(OH)3]- = 3.8 x 1014
21. What is the molar solubility of Mn(OH)2(s) in a solution that is buffered at pH 8.00 at 25 °C? The Ksp of Mn(OH)2 is 1.9 x 10- at 25 °C. The concentration of Pb in an aqueous solution is 5.5 x 103 M. What concentration of SO required to begin precipitating PbSO? The Ksp of PbSOa is 2.5 x 10 is 22. must be added to 1,0 L of 0.0180 M Pb2 (aq) to 23. What mass of KCl...
Question 12 7 pts Given the following Ksp values, if a solution contains 0.100 M each of Cu2+, Cd2+ and Sc3+, which ion would be present in a precipitate last if NaOH is slowly added to the solution? Ksp Cu(OH)2 = 2.2 x 10-20 Ksp Ca(OH)2 = 7.2 x 10-15 Ksp Sc(OH)3 = 8.0 x 10-25 Cd2+ All three precipitate out at the same time None of them would precipitate O Scat O Cu²
What is the OH ion concentration in a 4.8 x 10-2 M KOH solution? 2.1 x 10-13 M 4.8 x 10-2 M 1.0 x 10-7 M 4.8 x 10-12 M What is E' for the following balanced reaction? Fe(s) + Cu2+(aq) Fe2+ (aq) + Cu(s) Standard Reduction Potential Half-reaction Fe2+ (aq) + 2e Fe(s) Cu2+ (aq) + 2e Cu(s) -0.44 40.34 O +.010 +0.78 0 -0.78 -0.1
What is the pH of a 0.0013 M Ca(OH)2 solution? Answer to 2 decimal places. A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) ↔ H+(aq) + A-(aq) A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is...
Question 16 of 24 Determine the pH of a buffer that is 0.55 M HNO2 and 0.75 M KNO2. The value of Ka for HNO, is 6.8 x 10-4 1 2 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. HNO3(aq) + H2O(1) H,O*(aq) + NO, (aq) Initial (M) Change (M) Equilibrium (M) RESET 2x 0 0.55 0.75 6.8.10 0.55. 2x 0.56 - 2x 0.75 + x 0.75 - X 0.55 -...