calculate the pH of a solution of 2.8x10^-2 M BaOH2 mixed with the same volume of 0.040 M HCl
calculate the pH of a solution of 2.8x10^-2 M BaOH2 mixed with the same volume of...
Question 8 (2 points) A 6.5-ml sample of a 0.11 M HCl(aq) solution was mixed with a 4.1-mL sample of a 0.70 M HCl(aq) solution. Calculate the pH of the mixture. Provide your answer to the correct number of decimal places. Your Answer: Answer Hide hint for Question 8 There is no reaction. You are simply mixing two solutions of the same acid. First calculate the molarity of the mixture and finally the pH of the mixture.
0.001 L of 3.0 M NaOH was mixed with 0.166 L of distilled water. 0.040 L of this solution was transferred into a beaker. 0.001 L of 3.0 M HCl was added to the beaker. Calculate the pH and [H+].
7.(6 pts) Calculate the pH, [OH], and pOHl of a 0.0035 M HCl aqueous solution: 8. (6 pts) What are the [Hs0'1, (OH], and poH in a solution with a pH of 3.82? 9. (6 pts) What are the [H:0'], [OH], and pH in a solution with a pOH of 11.75? pH = pOH= , [OH'] = POH ' [OH'] = 10. (6 pts) Calculate the [H30, [OH1, and pH a 0.040 M Ba(OH)2 solution. [OH-11- pH=
Calculate the pH of the following solutions: a) Calculate the pH of the solution obtained by mixing 20.00 mL of 1.00 M HCl with water until a volume of 2000 mL. b) Calculate the pH by mixing 5.00 mmol of HNO3 with 5.00 mmol of KOH, in a total volume of 1000 mL of solution c) Calculate the pH by mixing 5.00 mmol of C6H5COOH with 3.00 mmol NaOH, and bring up to volume 300 mL. d) Calculate the pH...
A solution of 0.200 M KOH (17.6 mL) is mixed with 45.9 mL of 0.143 M HCl. Assuming that the final volume is the sum of the initial volumes, calculate: (a) the molarity of the K+ cation (b) the molarity of the Cl- anion (c) the pH of the final solution (d) the pOH of the final solution
Calculate the pH of a solution if 75.0 mL of 0.195 M HBr is mixed with 75.0 mL of 0.195 M Ca(OH)2 at 25.0 °C. Note: assume the volumes of the solutions are additive. Show work.
Determine the pH of a solution when 24.1 mL of 0.029 M HNO, is mixed with 18.6 mL of A. 0.0060 M NaOH. pH = B. distilled water. pH = C. 0.0100 M HCl. pH = D. 0.072 M KOH. pH =
A 4.4-mL sample of a 0.14 M HCl(aq) solution was mixed with a 6.3-mL sample of a 0.68 M HCl(aq) solution. Calculate the pH of the mixture. Provide your answer to the correct number of decimal places. Your Answer: Answer Hide hint for Question 16 There is no reaction. You are simply mixing two solutions of the same acid. First calculate the molarity of the mixture and finally the pH of the mixture.
Calculate pH of 0.2 M solution of Tartaric acid. Calculate the volume of 1 M solution of NaOH required to neutralize 20 mL of 0.2 M tartaric acid solution (final pH should be 7). (pKa's of Tartaric acid are 3.0 and 4.4). 3.
Question 7 (2 points) A 3.0-ml sample of a 0.10 M HCl(aq) solution was mixed with a 4.8-mL sample of a 0.63 M HCl(aq) solution. Calculate the pH of the mixture. Provide your answer to the correct number of decimal places.