3. Which of the following will make a buffer? CHOOSE ALL THAT APPLY. For each choice show your work or explanation that led you to your conclusion. If you can show a "before and after" you should. 10 mols of NH3 +1 mol of NH,CI 10 mols of NH3 + 200 mols of NH.CI 10 mols of NH3 + 2 mols of NaOH 10 mols of NH3 + 20 mols of HCI 10 mols of NH3 + 5 mols of HCI O O O

3. Which of the following will make a buffer? CHOOSE ALL THAT APPLY. For each choice show your work or explanation that led you to your conclusion. If you can show a "before and after" you should. 10 mols of NH3 +1 mol of NH,CI 10 mols of NH3 + 200 mols of NH.CI 10 mols of NH3 + 2 mols of NaOH 10 mols of NH3 + 20 mols of HCI 10 mols of NH3 + 5 mols of HCI O O O

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 95AP

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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Methyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?
Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).
Consider a buffer solution comprised of HF and F. The K₂ of HF is 6.3 x 10-4. If the pH of the buffer solution is 2.96 and [HF] = 0.115 M, how many moles of F* are present? The volume of the buffer solution is 426 mL. Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Answer:
Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of the NaFor solution should you add to 20 mL of the 0.10 M HFor solution to make your buffer?
you need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. if you start with 0.52 M NH4Cl solution, what concentration of NH3 will you need to start with. Kb for NH3 is 1.8x10^-5. Answer in two decimals and with units.
This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. H3C HO, H3C O`Na* H3C O Nat HO a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added. b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they? 10:2 11/28 hp fg f9 to
The following question refers to the buffer system: A 1.0-liter solution contains 0.35 M HNO2 and 0.45 M NANO2. If one adds 0.20 liters of 0.25 M HCl to the solution, what will be the pH? (K, for HNOzis 4.0 x 104). Moving to another question will save this response. MacBook Air F6 20 F3 D00 F5 F4 esc F1 F2 %23 %24 6. 7. #3 2.