= - A solution made with 24.3 grams of a diprotic acid, (Kal 4.68e-04; Ka2 = 7.74e-07) dissolved in 189 mL of solution, was titrated with 1.280 M NaOH. Calculate the pH at the first equivalence point: O (a) 3.330 ○ (b) 6.111 O (c) 4.721 O (d) 3.721 (e) 5.721
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- What is the pH of a solution of a freshwater solution at 25C containing 3mM DIC = H2CO3 + HCO3- + CO3^2? ( Please type answer note write by hend )ITTL/ What is the pH of 92.9 mL of a solution which is 0.29 M in NaCN and 0.61 M in HCN? For HCN use K₂ = 4.9x10-10. Your Answer:Old MathJax webview The total amount of base in a water sample can be determined by titration with standard acid, and is usually reported as the alkalinity, in equivalents of acid per liter (eq/L). If the alkalinity of a carbonate-containing samples is 1.0 ×10-3 eq/L, and the pH is 7.0, what are the concentrations of OH-, CO32-, HCO3-, and H2CO3? do it correctly. I will rate it
- . In a titration experiment, the pH of the vinegar used was found to be 2.45 which is equivalent to 0.800 M. Calculate the volume of vinegar needed to prepare 100 mL solution with a formality equal to 0.100 M.?? b. What glassware will be used in preparing the 100 mL solution ???An aqueous solution is prepared by mixing 50 mL of 2.0M KHPO4 and 25 mL of 2.0M K2HPO4 ,to a final volume of 200 mL/ What is the pH of the resulting solution? (Information the you may need: pKa H3PO4 = 2.15; pKa H2PO-4 = 6.82; pKa HPO4 2- = 12.38) a. 2.45 b. 6.52 c. 12.08 d. 6.82 e. 7.12"M" in .25M represents what? Question 4 options: Concentration None of the above Color pH
- Quinine (C20H24O2N2) is a water-soluble base that ionizes in two stages, with Kb1 5 3.31 × 10-6 and Kb2 5 1.35 × 10-10, at 25°C. Calculate the pH during the titration of an aqueous solution of 1.622 g of quinine in 100.00 mL of water as a function of the volume of added 0.1000 M HCl solution atthe following volumes: 0,3 Alice's pH meter broke and will only report [OH−]. What is the pH of a solution with a measurement of 1.122 mM?What is the pH of a 80.080.0 mL solution which is 0.290 M in IO− and 0.490 M in HIO? The Ka for HIO is 2.3×10−11
- Give typed full explanation Solution A is prepared by adding 50 ml of 0.3M hypochlorous acid solution to 50 ml of 0.2M of sodium hypochlorite solution. Calculate the pH change when 10 ml of a 1.00 M hydrogen bromide solution is added to 100 ml of solution A. Assume that volumes are additive.Phenolphthalein has a pKa of 9.7. It is colorless in its acid form and pink in its basic form. For each of the values of pH, calculate [In-]>[HIn] and predict the color of a phenolphthalein solution. a. pH = 2.0 b. pH = 5.0 c. pH = 8.0 d. pH = 11.0A solution is made by mixing 50.0 mL of a stock solution of 2.0 M K2HPO4 and 25.0 mL of a stock solution of 2.0 M KH2PO4. The solution is diluted to a final volume of 200.0 mL. What is the pH of the resulting solution given that the pKa of H2PO4- is 6.82?