Bundle: Introduction to General, Organic and Biochemistry, 11th + OWLv2, 4 terms (24 months) Printed Access Card
11th Edition
ISBN: 9781305705159
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
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Chapter 8.11, Problem 8.11P
Problem 8-11
What is the pH of a boric acid buffer solution containing 0.25 moI/L of boric acid, H3BO3 and 0.50 mol/L of its conjugate base? See Table 8-3 for the pKaof boric acid.
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Titration Problem
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Question 5
Which of the following mixtures would result in a buffered solution?
Mixing 100.0 mL of 0.100 MHC1 with 100.0 mL of 0.100 M NaOH.
Ⓒ Mixing 100.0 mL of 0.100 MNH3 (K=1.8 x 105) with 100.0 mL of 0.100 M NaOH.
Mixing 100.0 mL of 0.100 MHCI with 100.0 mL of 0.100 MNH3; (K=1.8×10)
Mixing 50.0 mL of 0.100 MHCI with 100.0 mL of 0.100 MNH3 (K₂=1.8 × 10-).
O At least two of the above mixtures would result in a buffered solution.
Problem 3A buffer made from which one of the acids below would be the best for a pH of 4.642?a) H2CO3 , Ka = 4.30e-7b) H2S, Ka = 9.10e-8c) CH3COOH , Ka = 1.75e-5d) H3PO4 , Ka = 7.52e-3
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- Titration Problemarrow_forwardChemistry practice questionarrow_forwardEXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.arrow_forward
- Problem 8-8 The [OH-] of a solution is M. What are the pOH and pH of this solution?arrow_forwardSaved 3 attempts left Check my work Be sure to answer all parts A 10.0-mL solution of 0.870 M NH, is titrated with a 0.290 M HCl solution. Calculate the pH after the following additions of the HCI solution: (a) 0.00 mL (b) 10.0 mL (c) 30.0 mL (d) 40.0 mL ( Prev 7 of 12 Next > MacBook Proarrow_forwardStudy guide answer is 4.77 for part 2 please show steps thanksarrow_forward
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