Concentration of 0.69mol/Lof the following Salts are dissolved in 100ml water1.3g(seperately and neutralized with either hydrochloric acidSodium hydroxide solution (both with aDecide for each salt, which solution you need for the neutralizationCalculate the volume of the solution needed for neutralization andCalculate the PH of the neutralized solutionc)LICNPka ₂ (H₂ 504) = 1.92, PKa (Har) = 9.40конa) NaHSON b) KOHPka₁ (H₂SO4) = -3,or

Given is a list of salts: Mass of the salts: Volume of water=Concentration of Concentration of To…

1. •3g of the following Salts are dissolved in 100ml water (Seperately and neutralized with either hydrochloric acid Concentration of 0.69mal/L Sodium hydroxide solution (both with a need for the neutralization you Decide for each salt, which Solution Calculate the volume of the solution needed for neutralization and Calculate the PH of the neutralized Solution or a) NaHSON b) KOH c) LicN кон Pka, (H₂SO4) = -3, Pkaz (#₂504) = 1.92. Pka (HCN) = 9.40

1. •3g of the following Salts are dissolved in 100ml water (Seperately and neutralized with either hydrochloric acid Concentration of 0.69mal/L Sodium hydroxide solution (both with a need for the neutralization you Decide for each salt, which Solution Calculate the volume of the solution needed for neutralization and Calculate the PH of the neutralized Solution or a) NaHSON b) KOH c) LicN кон Pka, (H₂SO4) = -3, Pkaz (#₂504) = 1.92. Pka (HCN) = 9.40

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A solution is made by adding 0.320 g Ca(OH)2(s), 35.0 mL of 1.10 M HNO3 and enough water to make a final volume of 75.0 ML. Assuming that all of the solid dissolves, what is the pH of the final solution?
4. Consider an aqueous solution of 1.50 M NH4Br. (Kb for NH3 = 1.8 x 10¹5) a) Which ion is pH neutral?; b) Which ion acts as an acid? c) Write a single net ionic equation to show that the solution is acidic. d) Calculate the pH the solution.
| To prepare a buffer solution of pH 3.50, the best acid choice is То + . Consequently, the buffer capacity is from to Suppose that the buffer solution changed its pH value following addition of acid or base. Someone would say the buffer solution is not a good buffer, if pH is
a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a solution which is 0.40 M in NH4+ and 0.40 M in NH3? The Kb of NH3 is 1.8 x 10-5. The correct answer should be reported to two places past the decimal. b) Caculate the pH of a solution prepared by mixing 84.7 mL of a 0.25 M aqueous aniline solution (C6H5NH2, Kb = 4.3 x 10-10) with 100. mL of a 0.11 M aqueous nitric acid solution. Your pH should be reported to two places past the decimal point.
When 25.0 mL of 0.200 M hydroiodic acid and 25.0 mL of 0.200 M ammonia are combined, the pH of the resulting solution will be : ..... fill in the blank 1A. Less than 7B. Equal to 7C. Greater than 7
Consider a saturated solution containing Ca(NO3)2 at 25°C. not enough info/greater than 7/ less than 7/ equal to 7 This solution would be choose your answer... The pH of the solution would be choosehtour answer. choose your answer. acidic/neutral/not enough info is given/ basic
You add 7.50 mL of 0.050 M NaOH to 50.00 mL of pure water, and to this mixture you then add 1.50 mL of 0.200 HCl. What will be the pH of the resulting solution? A) 11.10 B) 2.11 C) 7.00 D) 11.89 E) 2.49
... 2@ 48 TO Time left 0:24:03 Consider a solution initially containing 0.40 mol fluoride anion (F) and 0.30 mol of hydrogen fluoride (HF). If 0.40 mol of HCl are added to this solution, which of the following statements is/are FALSE? Addition of 0.40 mol of HCI will lover the pH of solution by 0.4 unit. O You'll essentially have a weak acid solution situation, with 0.7 mol HF at the end. O You will still have a buffer solution at the end, since you'll still have significant amounts of both weak base and conjugate weak acid. You will no longer have a buffer solution, since all of the buffer capacity was exhausted. The pH will have shifted to a lower pH.
Calculate the pH of each of the following strong acid solutions.(a) 0.00751 M HIO4pH = (b) 0.529 g of HCl in 42.0 L of solutionpH = (c) 30.0 mL of 3.40 M HIO4 diluted to 3.00 LpH = (d) a mixture formed by adding 28.0 mL of 0.00747 M HIO4 to 23.0 mL of 0.00771 M HClpH =
8.) A solution is made where 0.878 moles HCl is added to water that has a total volume of solution of 1855mL. What is the pH of the solution. НС(аq) — н' (аq) + CГ(aq)
It was found that 36.06 mL of HNO3 solution are needed to react completely with 25.0 mL of 0.19 M LIOH solution that has a pH of 13.29. What is the molarity of the HNO3 solution? [HNO3] = M
It was found that 27.53 mL of HNO3 solution are needed to react completely with 20.0 mL of 0.00026 M LIOH solution that has a pH of 10.42. What is the molarity of the HNO3 solution? [HNO3] = i M