6.7.8.For a particular application in my lab, we often need to make a formic acid buffer. The chemical formula for formic acid is HCO₂H.To make this buffer, let's say we start with 2.53 M sodium formate in 1 L of water (and assume 1L of volume throughout this problem).5.2.3. (4.1.Using the chemical formula information above, show the chemical reaction of formate with water to form products (hint: whatpart of the sodium formate reacts with the water?) Make sure you include the phases of matter.What is the value of the equilibrium constant for this reaction?What is the pH of the solution right now?Let's say we add HCl, show the reaction that would occur (what part of the HCI reacts with what part of the equilibrium reactionoutlined in part 1?)Let's say we add 0.45 moles of HCI. What is the resulting pH now?Ok, to the solution in #5 above, after we add the HCI, we now add 0.23 mol NaOH. Identify the component in the solution withwhich the NaOH will react.What is the new pH of the solution described in #6?At which stage in here (Identify a number 1, 4, or 6) does this solution become a buffer and briefly describe why.

ical formula for formic acid is HCO₂H. To make this buffer, let's say we start with 2.53 M sodium formate in 1 L of water (and assume 1L of volume throughout this problem). 1. Using the chemical formula information above, show the chemical reaction of formate with water to form products (hint: what part of the sodium formate reacts with the water?) Make sure you include the phases of matter. 2. What is the value of the equilibrium constant for this reaction?

ical formula for formic acid is HCO₂H. To make this buffer, let's say we start with 2.53 M sodium formate in 1 L of water (and assume 1L of volume throughout this problem). 1. Using the chemical formula information above, show the chemical reaction of formate with water to form products (hint: what part of the sodium formate reacts with the water?) Make sure you include the phases of matter. 2. What is the value of the equilibrium constant for this reaction?

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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10) A buffer solution with a volume of 775.0 mL is made with 0.225 mol of HC2H302 and 0.100 mol NaC2H3O2. If 2.30 g of NaOH is added without changing the volume of the solution, what is the pH of the resulting solution? The pk, of acetic acid is: 4.74. (4.71)
100.0 mL of HCI required 5.831 g Mg(OH)2 to titrate. The molar mass of Mg(OH)2 is 58.31 g. What is the concentration of the HCI ? The neutralization equation is 2 HCI + Mg(OH)2 MgCl₂ + 2 H₂O There is enough information to calculate the moles of Mg(OH)2 mol Mg(OH)2 -): (5.831 g Mg(OH)₂ (- g Mg(OH)₂ Then use stoichiometry to convert moles of Mg(OH)2 into moles of HCI mol HCI concentration a. acid i. 0.2000 mol Mg(OH)2 (-- mol Mg(OH)2 We now can calculate the concentration of HCI since we have both the moles of HCI and the volume of HCI mol HCI p. 0.01000 b. base c. HCI NaOH j. 1.000 k. 0.005000 q. 0.001000 L HCI r. 58.31 e. NaCl I. 100.0 f. H₂O m. 0.1000 s. 5.831 g. 25.00 mol Mg(OH)2 mol/L n. 0.05000 h. 0.02500 mol HCI o. 2.000
5. 6. 7 8 10 11 12 13 14 1 A chemistry graduate student is given 100. mL of a 0.60M dimethylamine ((CH,), NH) solution. Dimethylamine is a weak base with K,=5.4 × 10 ". What mass of (CH,, NH,Br should the student dissolve in the (CH,), NH solution to turn it into a buffer with pH =11.05? db You may assume that the volume of the solution doesn't change when the" (CH, NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. Submit Assignment Continue MacBook Air F10 FI F8 F9 000 F7 80 F6 D00 F4 F5 esc F3 FI * @ # $ 9
9) a) Which of the following solutions would make a buffer? NaH2PO4/H3PO4 HCI/NaCl NH3/NHẠCI NaOH/H20 HC;H;O2/NAC2H3O2 b) What is the pH of a buffer that contains 0.375 M HF and 0.250 M NaE? The pkaof Hf is 3.14. (2.96)
(10.2) Calculate the fluoride ion concentration and pH of a solution that is 0.20 M in HF and 0.10 M in HCl. Ka 6.8 × 10¬4
10) A buffer solution with a volume of 775.0 mL is made with 0.225 mol of HC2H3O2 and 0.100 mol NaC2H3O2. If 2.30 g of NaOH is added without changing the volume of the solution, what is the pH of the resulting solution? The pKa of acetic acid is: 4.74. (4.71)
10.110 A 0.312 M KOH solution is used to titrate 15.0 mL of an H,SO, solution. (10.7) a. Write the balanced chemical equation. b. What is the molarity of the H,SO,4 solution if 28.2 mL of the KOH solution is required?
(5.7: Similar to For practice 5.11)The titration of a 20.0 mL sample of an H₂SO4 solution of unknown concentration requires 18.88 mL of a 0.203 M KOH to reach the equivalence point. What is the concentration (in M) of the unknown H₂SO4 solution? (Hint: Write the balanced reaction equation first.) O 0.0958 M O 0.383 M O 0.767 M O 0.192 M
4. 5. OH + HCI I strong acid catalyst
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