A solid monoprotic acid (MM = 200. g/mol) was used to standardize a NaOH solution. If in a different trial, a solid diprotic acid (MM = 200. g/mol) was used instead, how would this affect the amount of NaOH added and its molarity? The amount of NaOH is halved and the M of the acid is the same The amount of NaOH is doubled and the M of the acid is the same The amount of NaOH is the same and the M of the acid is the same The amount of NaOH is halved and the M of the acid is halved The amount of NaOH is doubled and the M of the acid is doubled O O O O O

A solid monoprotic acid (MM = 200. g/mol) was used to standardize a NaOH solution. If in a different trial, a solid diprotic acid (MM = 200. g/mol) was used instead, how would this affect the amount of NaOH added and its molarity? The amount of NaOH is halved and the M of the acid is the same The amount of NaOH is doubled and the M of the acid is the same The amount of NaOH is the same and the M of the acid is the same The amount of NaOH is halved and the M of the acid is halved The amount of NaOH is doubled and the M of the acid is doubled O O O O O

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...

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An undergraduate research student wishes to create a system that mimics human blood (pH = 7.4). The student chose as the model system to use a buffer solution of sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4, Ka = 4.2 × 10-13). A) Which of the components of the buffer solution is the acid? B) Using the Henderson Hasselbalch equation, calculate the mole ratio of Na2HPO4/NaH2PO4 the student needs to use. C) To approximate the human condition of blood alkalosis (where the pH of blood rises to 7.6, which is usually lethal), how much base will the student need to add to the buffer?
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )
Answer the following questions about a titration between 20.0 mL of a weak base (Kb= 4.7*10-6) and 0.150 M hydrochloric acid. A.What is the concentration of the weak base solution if it requires 26.67 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of bruhmophenol is ~ 4.9 and the pKa of thymol blue ~ 9.2. Which indicator would be best to use in the titration
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Part A When a solution contains a weak acid and its conjugate base or a weak base and its conjugate acid, it will be a buffer solution. Buffers resist change in pH following the addition of acid or base. A buffer solution prepared from a weak acid (HA) and its conjugate base (A) is represented as What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant K of HA is 5.66 x 10-7. Express the pH numerically to three decimal places. HA(aq) = H+ (aq) + A-(aq) • View Available Hint(s) The buffer will follow Le Châtelier's principle. If acid is added, the reaction shifts to consume the added H+, forming more HA. When base the base will react with Ht, reducing its concentration. The reaction then shifts to replace H+ through the dissociation of HA into H+ and A. In both instances, H+] tends to remain constant. added, V AZO The pH of a buffer is calculated by using the Henderson-Hasselbalch pH = equation: pH =…
Added strong base: NaOH solution OH Acetic acid/acetate buffer N-7 Mix OH +CH;COOH CH;COO" + H Added Weak acid in buffer cak base strong base Conjugate created from buffer CH.COOH What is the net ionic equation for the reaction that occurs when small amounts of sodium hydroxide are added to HOCI/NAOCI buffer solution? Na + HOCI O NAOH + HOCI NaCl + OH™ H2O + NaCl OH+ OCI HOCI + 02- OH +HOCI H2O + OCI" H + HOCI H2 + OC
A student prepared 100.0 mL of a buffer in the lab that contains 0.300 M of a weak acid, HA, and 0.200 M of its conjugate base, NaA. The student then added 1.0x10 moles of NaOH to the buffer. a) Write down your student name and number b) Write down how the student calculated the final moles of A and HA after adding the NaOH: moles A finl =2.0x102 mole - 1.0x10-3mole moles HA na = 3.0x102mole +1.0x10-3mole c) There is an error in their formula. Identify the error d) Calculate the correct final moles of A and HA