4: Stoichiometryin acid base reactions/titrations4. 25.00 mL a phosphoric acid solution is titrated with 0.250 M Sr(OH)2 solution. If ittakes 32.00 mL of Sr(OH)2 to reach end point, what's the molarity of phosphoricacid?5. 50.0 mL of a sulfuric acid solution of unknown concentration is titrated with a 0.100M sodium hydroxide titrant solution. The end point is reached after 40.0 mL oftitrant are added. Calculate the molarity of the sulfuric acid solution.islom ynsm woll6. 50.00 mL of 0.100 M H₂SO4 acid solution is being titrated with 0.250 M NaOHsolution. How many mL of NaOH will be needed to reach the endpoint?10.epi192000borbyn

Answered: Image /qna-images/answer/5e1edea5-170e-4888-a559-3a4cbb2b3525.jpg

Answered: 4. 25.00 mL a phosphoric acid solution…

4. 25.00 mL a phosphoric acid solution is titrated with 0.250 M Sr(OH)2 solution. If it takes 32.00 mL of Sr(OH)2 to reach end point, what's the molarity of phosphoric acid?

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

6
A 27.56 mL portion of a 0.337 M solution of hydrochloric acid, a monoprotic acid, is to be titrated with a standarized 0.411 M solution of KOH. What is the expected volume in milliliters of the KOH solution needed to reach the phenolphthalein end point? Report your answer with a precision of two decimal places.
25.0 mL of a Ba(OH)2 solution are titrated with hydrochloric acid. If 12.10 mL of 0.0825 M HCl are needed to reach the endpoint of the titration, what is the molarity of the Ba(OH)2 solution? HCl (aq) + Ba(ОН)2 (аq)
Constant-boiling HCI can be used as a primary standard for acid-base titrations. A 50.00 mL sample of constant-boiling HCI with a concentration of 0.1020 M was collected and titrated to an endpoint with 40.29 mL of a Ba(OH)₂ solution. What is the molarity of the Ba(OH)₂ solution? concentration: M
For your titration, it took 17.91 mL of unknown NaOH to react with 0.223 g of KHP. What is the molarity of the NaOH?
4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100
What is the pH at the equivalence point in the titration of a 22.6 mL sample of a 0.398 M aqueous acetic acid solution with a 0.387 M aqueous barium hydroxide solution? pH =
24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid. Calculate the molarity of phosphoric acid.
A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)
6. Acid/base titration is a common method to determine the molarities of acids or bases, the molarity of certain salts can also be determined by titration. It took 22.34 mL of 0.5861 M HCl solution to neutralize 25.00 mL NaNO₂ solution. The acid- dissociation constant of HNO₂ is 4.511 × 10-¹. NaNO₂ + HCl → HNO₂ + NaCl Please answer the following questions. A What is pH of the NaNO₂ solution before titration? Hint, calculate the molarity of the NaNO₂ solution first. pH = Please provider your answer below. ( Check answer 7²² B. M HCl solution was added to the NaNO2 solution? pH = 00 0 Please provider your answer below. What is the pH when 12.78 mL of 0.5861 (0) Check answer C. What is the pH when 14.39 mL of 0.5861 M HCl solution was added to the NaNO₂ solution AFTER the equivalence point? pH = Please provider your answer below. 00 0 °C? pH= Please provider your answer below. Check answer What is the pH at equivalence point at 25 A → ← Check answer ← $ H $