1) Which one of the following combinations of solutions will NOT form a buffer solution? a. NaCl and NaCH₂COO b. NH4Cl and NH₂ c. KCN and HCN d. HNO₂ and CSNO₂ 2) a. Calculate the pH of a 100.0 mL buffer made by combining 0.24 M acetic acid (CH₂COOH, K₂= 1.8x105) and 0.15 M cesium acetate (CsCH3COO). Calculate the pH of the above solution after 3.59 mL of 1.0 M CSOH is added. Include a balanced chemical equation and change table (or equivalent work) below.

1) Which one of the following combinations of solutions will NOT form a buffer solution? a. NaCl and NaCH₂COO b. NH4Cl and NH₂ c. KCN and HCN d. HNO₂ and CSNO₂ 2) a. Calculate the pH of a 100.0 mL buffer made by combining 0.24 M acetic acid (CH₂COOH, K₂= 1.8x105) and 0.15 M cesium acetate (CsCH3COO). Calculate the pH of the above solution after 3.59 mL of 1.0 M CSOH is added. Include a balanced chemical equation and change table (or equivalent work) below.

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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8. a) Which of the following mixtures would result in a buffer solution? Very briefly explain why for each one. i. 100 mL of 0.1M sodium acetate (NaOAc) + 50 mL of 0.1M hydrobromic acid (HBr). 50 ml of 0.01M acetic acid (HOAC) + 150 mL of 0.01M sodium hydroxide (NaOH). ii. 100 mL of 0.02M sodium fluoride (NaF) + 50 mL of 0.02M potassium hydroxide (кон). 8. b) Calculate the pH of a buffer that was prepared by mixing 45 mL of 0.01M aqueous hydrocyanic acid (HCN, K, = 6.2 x 10ʻ1º) with 11 mL of 0.02M aqueous potassium hydroxide (KOH).
What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric acid/fluoride buffer with a pH of 4.25 from 1.25 M HF and solid potassium fluoride? The Ka for HF is 6.8×10–4.
2) Which of the following combinations of materials would result in a buffer solution?*100. mL of 1.0 M HCl + 50.0 mL of 1.0 NaCl*100. mL of 1.0 M HNO2 + 100. mL of 2.0 M NaNO2*100. mL of 1.0 M CH3NH2 + 100. mL of 0.50 M CH3NH3+*100. mL of 1.0 M HF + 50.0 mL of 1.0 M HClO
a Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOCI. Ka = 3.5x10-8 pH = 8.1 b In order for HOCI/KOCI buffer to have pH = pKa, would you add HCI or NaOH? pKa = 7.46 pH = 8.1 NaOH O HCI What quantity (moles) of HCI would you add to 1.0 L of the original buffer (0.20 M HOCI and 0.88 M KOCI) so that the resulting solution has pH = pKą? pka = 7.46 Quantity = mol Submit
a Calculate the pH of a solution that is 0.20 M HOC1 and 0.92 M KOCI. Ką = 3.5x10-8 pH = 8.16 b In order for HOCIKOCI buffer to have pH = pKa, would you add HCl or NaOH? pKa = 7.46 pH = 8.1 HC1 NaOH © What quantity (moles) of HCl would you add to 1.0 L of the original buffer (0.20 M HOC1 and 0.92 M KOCI) so that the resulting solution has pH = pKq? pKa = 7.46 Quantity mol
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.40 M NaH2PO4 and 0.60 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution? Provide your answer to 2 decimal places If the pH calculated in b was the blood pH of an actual patient, would you say this patient’s blood pH is within normal range or are they suffering from alkalosis or acidosis?
ALL ABOUT BUFFERS 1. All of the following combinations are not buffer solution, EXCEPT: a HI and NaI b NH3 and NH4Cl c HNO3 and NH4NO3 d HClO4 and NaClO4 2. Which of the following pairs can act as buffer? a CO2 / H2CO3 b Na2SO4 / H2SO4 c Na3PO4 / H3PO4 d NaCl / HCl 3. The pH of the buffer will NOT change after the addition of large amounts of water True False 4. A buffer is prepared using 0.085 Mformic acid (HCOOH) and 0.085 Msodium formate (NaHCOO). Which of the following statements is FALSE? a The addition of 0.02 M HCl will decrease the pH slightly b The addition of 0.02 M NaOH will increase the pH slightly c The formate ion can neutralize bases added to the buffer d The addition of 1.0 M HCl will cause the pH to drop significantly e Diluting the solution with pure water won't change the pH of the buffer 5. The following are true for buffer, EXCEPT:…
15. A buffer is prepared by mixing 2.50 g of benzoic acid (HC7H5O2) and 3.50 g of sodium benzoate (NaC7H5O2) in 1.00 L of water. The Ka for benzoic acid is 6.6 × 10-5 a. Find pH of buffer b. Find the pH of the buffer when 5.0 mL of 0.120 M HCl is added c. Find the pH of the buffer when 90.00 mL of 2.100 M HCl are added. Show all work and ICE table if applies.
A buffer is prepared from 60.0 mL of 0.100 M formic acid(HCOOH) and 40.0 mL of 0.100 M formate (HCOO --). What is thepH of the buffer solution ? K a of formic acid is 1.78 x 10 4
5, Which of the following pairs will not form a buffer when mixed together in an aqueous solution? a. Na2HPO4 and KH2PO4 b. HF and NaF c. NaCl and NaOH d. HOCl and NaOCl e. all of the above are buffers
What is the pH of a buffer made by combining 45.0 mL of 0.34 M nitrous acid and 60.0 mL of 0.48 M sodium nitrite? The Ka of nitrous acid, HNO2, is 4.5×10–4. a. 3.20 b. 3.62 c. 7.00 d.0.98