Accessibility Modev Don1. a. In a hospital laboratory, a 10.0 mL sample of gastricjuice obtained several hoursafter a meal was titrated with 0.1 M NAOH to neutrality; 7.2 mL of NaOH wasrequired. The patient's stomach contained no indigested food or drinks, thusassume no buffers were present. What is the pH of the gastricjuice?b. Lactic acid is produced and builds up in muscles during intense exercise andcauses painful, sore muscles. What is the pH of 0.6 mM lactic acid, pKa=3.86?1c. What is the pH of a mixture of equal volumes of 0.6 mM HCI and 0.4 mMNaOH?d. What is the pH of a mixture of equal volumes of 0.6 mM Lactic acid and 0.4mM NAOH?e. If the concentrations of HCl and NaOH are tripled in part c, by what factoF willthe pH be changed?f. If the concentrations of lactic acid and NaOH are tripled in part d, by what factorthe pH be changed?g. What is tihe rationale for the observed difference in pH as a function ofincreasing HCl and lactic acid concentrations?

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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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1. a. In a hospital laboratory, a 10.0 mL sample of gastricjuice obtained several hours after a meal was titrated with 0.1 M NAOH to neutrality; 7.2 mL of NaOH was required. The patient's stomach contained no indigested food or drinks, thus assume no buffers were present. What is the pH of the gastricjuice? b. Lactic acid is produced and buildsup in muscles during intense exercise and causes painful, sore muscles. What is the pH of 0.6 mM lactic acid, pKa=3.86? 1 c. What is the pH of a mixture of equal volumes of0.6 mM HCl and 0.4 mM NaOH? d. What is the pH of a mixture of equal volumes of 0.6 mM Lactic acid and 0.4 mM NaOH? e. If the concentrations ofHCl and NaOH are tripled in part e, by what factor will the pH be changed? f. If the concentrations oflactic acid and NaOH are tripled in part d. by what factor the pH be changed? 85°F Mostly cloudy 直

Recently graduated from the ESST programme in UWI, you land a job as a technical officer in the EMA. A proposal to allow an industry to release hydrochloric acid into a small lake crosses your desk; the proposal can only be approved if the pH of the water in the lake will remain within the regulated pH range of 6 – 9 after the hydrochloric acid has been released. To assist the EMA in making their decision, the buffer capacity of the lake water is determined. Buffer capacity is a parameter similar to alkalinity, in that it indicates how much acid or base can be added to the water to achieve a pH change of 1 unit. (a) The buffer capacity of the lake is measured, and is found to be 7.95×10-4 mol/L. Given that the volume of the lake is 5.0×1010 m3, how many moles of H+can the lake absorb before the pH of the water drops by 1 pH unit?
A 1.451.45 L buffer solution consists of 0.1590.159 M butanoic acid and 0.3320.332 M sodium butanoate. Calculate the pH of the solution following the addition of 0.0620.062 moles of NaOHNaOH. Assume that any contribution of the NaOHNaOH to the volume of the solution is negligible. The ?aKa of butanoic acid is 1.52×10−51.52×10−5.
Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base are mixed in equimolar proportions? Acid NH4* (from ammonia) HC₂H3O2 (acetic acid) HF (hydrofluoric acid) CH3CH₂NH3 (from ethylamine) acetic acid. b) ethylamine c) ammonia d) hydrofluoric acid e) none Ka 5.69 10-10 1.75 10-5 6.810-4 2.12 10-11
The pH of unbuffered water, such as rain, is decreasing consistently over time as atmospheric CO2 concentrations increase. a) What will be the atmospheric CO2 level (in ppm) when the pH of rain water reaches 5.50 at 25 °C? b) What would be the pH of buffered water (over CaCO3 limestone at 25 °C) at the CO2 level in part a)? c) Determine the concentrations of HCO3– and CO32– ions in the buffered water of part b) and then determine the alkalinity of the solution in ppm CaCO3.
7,8
Define the term Buffer-Capacity?
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
A 100 mL buffer solution that is pH 8.06 buffer is prepared by first adding 0.45 grams of RNH2 (121.1 g/mole) into a beaker. To make the solution, how many mL of a stock solution of 1.0 M R-NH3+ solution should be added to the beaker before diluting to 100 mL?
Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI
a) A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol) b) 10 mL is accidentally spilled into the buffer solution from part a. Determing the new pH of the solution.
100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.

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