You are instructed to create 100 mL of a 0.05 M Acetate buffer with a pH of 3.8. You have Glacial Acetic acid (17.4M,Ka=1.8e-5)) and the sodium Acetate NaC2H302, available. (Enter all numerical answers to three significant figures.) Copy the results into your lab notebook for use in class. How many grams of Sodium Acetate are needed for the buffer?

You are instructed to create 100 mL of a 0.05 M Acetate buffer with a pH of 3.8. You have Glacial Acetic acid (17.4M,Ka=1.8e-5)) and the sodium Acetate NaC2H302, available. (Enter all numerical answers to three significant figures.) Copy the results into your lab notebook for use in class. How many grams of Sodium Acetate are needed for the buffer?

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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4. You need to make a buffer with pH as close to 10.00 as possible. Two sets of weak acids and conjugate bases, with the Ka values, are listed below. Which of the two sets would be the best choice? You want a pka close to the pH. Explain your reasoning. CH:COOH/CH;coo HCO; /CO,2- Ka = 1.80 x 10s Ka = 2.14 x 10-10 %3D %3D 5. 5 drops of a strong base (0.1 M concentration) was added to a buffer (pH = 7.0), with no apparent change in pH. An additional 5 ml of this strong base was added, and the pH of the solution increased to 13.0. Explain why there was no apparent change in pH in the %3D first case, but a marked change in pH in the second case.
Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places)
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?
Consider a beaker containing 50 mL of 0.20 M of a weak acid (HA) with a pKa of 5.25. How many mL of 0.20 M NaOH (a strong base) should be added to the beaker make a buffer with pH 5.83? How many mL of 0.20 M A- (the weak conjugate base of the weak acid, HA) should be added to the beaker make a buffer with pH 5.83?
Enter your answer in the provided box. Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate (NaHCO3) is always 0.31 M, but the concentration of sodium carbonate (Na₂CO3) corresponds to the following value: 0.31 M. (K for HCO3 is 5.6 × 10-11.) Report your answer to four significant figures.
A through d
1. Suppose you have a solution of 25.0 ml pure water. You add add three drops of 1.0 M HCI to the pure water solution. Find the pH change of solution after addition of HCI. 2. Find the pH change of 25.0 ml pH buffer (0.20 M HAC + 0.20 M NaAc) after adding three drops of 1.O MM HCI. Use the editor to format your answer
Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with KOH in water. If 40.00 mL of the KOH solution is required to reach the equivalence point, what will the pH of the solution be after only 20.00 mL of the KOH solution has been added? Group of answer choices 1.80 2.91 3.74 4.56
3 NEXT > < PREV 1 2 Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 6.3 × 10-5 RESET [0] [21.5] [37.7] [0.176] [0.261] [0.880] [1.31] [0.178] [0.888] [x] [2x] [21.5-x] [37.7+x] [0.176-x] [0.261 + x] [0.880 - x] [1.31 + x] [0.178 + x] [0.888 + x] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Ka (Part 2), determine the pH of the buffer solution. pH = RESET 0 4.2 x 10-5 6.23 4.37 2.4 × 10-11 7.77 9.63 0.880
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 make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 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 with 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 in the normal range or are they suffering from alkalosis or acidosis?
part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What would be the pH of this solution? part b: How many milliliters (mL) of 19.00 M NaOH are need to adjust the pH of this buffer to pH 10.00? Please answer part b
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