26. Calculate the pH of 0.25 M HNO2 (K. = 4.0 x 10). Justify any assumptions...
26. Calculate the pH of 0.25 M HNO2 (K, -4.0 x 10). Justify any assumptions made regarding you (hint: check assumption with % ionization). Show all work for full credit. (6 pts)
calculate the ph of 0.25 M HNO2 (Ka= 4.0 * 10^-5)
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate the concentration of HNO2 and its conjugate base in a 0.025 M HNO2 Solution. Please please show all work!
6. Calculate the pH of 0.010 M HNO2 solution. The K, for HNO2 is 4.6 x 104 Answer: pH = 2.72
Calculate the pH of the following acid–base buffers. Be sure to state and justify any assumptions you make in solving the problems. a. 100.0 mL of 0.025 M formic acid and 0.015 M sodium formate b. 50.00 mL of 0.12 M NH3 and 3.50 mL of 1.0 M HCl c. 5.00 g of Na2CO3 and 5.00 g of NaHCO3 diluted to 0.100 L 4. (10 Points) Calculate the pH of the buffers in problem 3 after adding 5.0 mL of...
II. Problem Solving. Show all work, thoroughly and completely Do not omit any steps. No credit will be given for illegible, ambiguous, or unclear work. CIRCLE OR UNDERLINE YOUR FINAL ANSWERS 11. Calculate the pOH and pH of a 0.025 M HF. K, (HF)= 3.0 x 10 (Hint: Assume the change is small) (15 points) 12. Find the [Hj0') and percent ionization of a 2.5 M HNO2 solution according to the equation below. (Hint: Assume the change is small) (15...
2. What is the pH of a solution which is 0.25 M KHCO, if the K, for HCOs is 2.4 x 10*2 Calculate the concentrations of НЗО", ОН, NHs, and cr in a solution prepared by dissolving 535 g of NH4CI in enough water to make 5.00 × 102 miL of solution at 25 °C., for NII is 1.8 x io-s. Hint: Is the given ionization constant for NHs the correct value to use in your calculations?) 3.
Calculate the pH of the following acid–base buffers. Be sure to state and justify any assumptions you make in solving the problems. a. 100.0 mL of 0.025 M formic acid and 0.015 M sodium formate b. 50.00 mL of 0.12 M NH3 and 3.50 mL of 1.0 M HCl c. 5.00 g of Na2CO3 and 5.00 g of NaHCO3 diluted to 0.100 L
5.) Calculate the concentrations of all the species and the pH in 0.25 M hypochlorous acid, HOCL. For HOCL, Ka=3.5x10^-8 6.) the pH of a 0.115M solution of chloroacetic acid, CICH2COOH, is measured to be 1.85. Calculate the Ka for this monoprotic acid Calculate the concentrations of all the species and the pH in 0.25 M hypochlorous acid, HOCI. For HOC, Ka :3.5 x 108. .) The pH of a 0.115M solution of chloroacetic acid, CICH2COOH, is measured to be...
1) The ionization constant for NH4+ is K = 5.8 x 10-10 at 25oC. It is in a reversible equilibrium with ammonia and H+. NH4+ --> NH3 + H+ where, H+ + NH3 --> NH4+ with a k1 = 2.300 x 1010 M-1 s-1 A temperature jump from 20oC to 25oC is made on a 0.1 M NH4Cl solution at pH 6. Calculate the relaxation time in microseconds for the reaction, assuming that the mechanism is given by the ionization...