Need help with this ASAP QUESTION 7 What is the pH of 0.15 M solution of...
7. What is the pH of a solution made by mixing 29.00 mL of 0.15 M acetic acid with 29.00 mL of 0.15 M KOH? Assume that the volumes of the solutions are additive. Ka= 1.8 x 10-5 for CH3CO2H oka-loa 8x10
Question 14 QUESTION 13 What is the final pH if 36.0 mL of 0.15 M of NaOH is added to 90.0 mL of 0.80 M acetic acid? Ky for acetic acid is 1.8 x 10-5, CH3COOH(aq) + OH(aq) + H2O(l) + CH3COO (aq) Note: No quadratic. Need ICE table QUESTION 14 The Ksp for Mg(OH)2 is 1.8 x 10-11. What is the concentration, in M, of OH ions in a saturated solution of Mg(OH)2? 52x104 1.7×104 3.3 x 10-4 26x104
Question 13 QUESTION 13 What is the final pH if 36.0 ml. of 0.15 M of NaOH is added to 90.0 ml of 0.80 M acetic acid? Ky for acetic acid is 1.8 x 10-5 CH3COOH(aq) + OH" (aq) + H200) + CH3COO(aq) Note: No quadratic. Need ICE table QUESTION 14 The Ksp for Mg(OH)2 is 1.8 10-11What is the concentration, in M, of OH ions in a saturated solution of Mg(OH)2? 5.2 x 10-4 1.7×104 3.3 x 104 2.6x104
8. What is the pH of a solution made by mixing 29.00 mL of 0.15 M acetic acid with 39.00 mL of 0.15 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 x 10-5 for CH3CO2H.
Calculate the pH of a 0.15 M CH3COOK solution. (Ka for acetic acid = 1.8 × 10−5.)
Which one of the following solutions has the lowest pH? A. a 0.1 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) B. a 0.1 M solution of ammonium chloride, NH4Cl(s) (Ka (NH4+) = 5.6 x 10-10) C. a 0.01 M solution of acetic acid, CH3COOH (Ka = 1.8 x 10-5) D. a 0.01 M solution of formic acid, HCOOH (Ka = 1.8 x 10-4) E. a 0.1 M solution of acetic acid, CH3COOH (Ka = 1.8 x...
Q: What is the pH of a solution containing 0.125 M KH2PO4 and 0.175 K2HPO4 Ka (H2PO4-) = 6.2 x 10-8 Ka (HPO42-) = 4.8 x 10-13 Q: A 0.15 M solution of a weak acid is 3.0 % dissociated. What is the Ka of this acid? Q: A solution of aspirin was prepared that is 0.16 M. The pH of this solution was measured to be 2.43. What is the Ka of aspirin? Q: A solution of formic acid...
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...
What is the pH of a buffer solution containing 0.13 M HF and 5.0×10−2 M NaF? What is the pH of a buffer solution containing 1.0×10−2 M HF and 0.16 M NaF? Using the table given below for Ka values, compare the pH of an HF buffer that contains 0.13 MHF and 5.0x10-2 M NaF with another HF buffer that contains 1.0x10-2 MHF and 0.16 M NaF. Ka and K b values for selected weak acids and bases HF Acid...
I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer, will not produce a pH o 9.00" 1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...