Question 7 (2 points) A 3.0-ml sample of a 0.10 M HCl(aq) solution was mixed with...
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.
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.
1) 7. 10.0 mL of 0.10 M HBr is mixed with 10.0 mL of 0.10 M HCOOH. What is the pH? 2) 15. Calculate the pH of a solution containing 2.5 x 10 –2 mol of nicotinic acid (a monoprotic acid dissolved in 350 mL of water. ( K a = 1.1 x 10 -5 ) 3) A 1.0 L buffer solution is made up of 0.15M NaF and 0.20 M HF ( pK a = 3.17) . 0.05 mol...
A 10.0 mL sample of 0.25 M NaOH(aq) is titrated with 15.0 mL of 0.10 M HCl(aq) (adding HCl to NaOH). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Assume that the volumes of the solutions are additive. 1)After adding the HCl solution, the mixture is [select one](before, After, at) the equivalence point on the titration curve. 2)The pH of the solution after adding HCl is [select one](7.00,1.40,11.00,12.60).
A 25.0 mL sample of 0.10 M sodium benzoate is titrated with 0.10 M HCl(aq). What is the pH after the addition of 25 mL of HCl(aq)? (K) of CoH;CO2- - 1.6 * 10-10) O pH <7 and > 3 O pH>10 O pH > 7 and <10 O pH=7 O pH< 3
Question 5 (2 points) Calculate the pH of a solution labelled 7.1 M HCl. Provide your answer to the correct number of decimal places. Your Answer: Answer
1) Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq) and 100.0 mL of 0.20 M NaOH(aq). 2) Calculate the pH of an aqueous solution made by mixing 100.0 mL of 0.40 M NH4Cl and 50.0 mL of 0.40 M NaOH. The pKa of NH4+ is 9.24.
2. A 25.0 mL sample of 0.12 M HBr is mixed with 15.0 mL of 0.10 M KOH. Calculate the pH of the mixture. Assume the volumes are additive.
Question 6 1 pts A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid. Ko of NH3 is 1.8 x 10-5 Henderson-Hasselbalch equation: pH = pka + log og HCI NH, NH3- Parta): 1) After adding 10 mL of the HCl solution, the mixture is (Select] the equivalence...
A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.14 MNH 3. What is the resulting pH? (Kb for NH 3 1.8 x 10-5) Oa. 1.52 Ob. 10.96 Oc. 3.04 Od. 1.70 Oe. 12.30