Buffer, its a homework for chemistry and i need it as soon as possible and thanks? 2. A 55-year-old patient was admitted to the hospital with shortness of breath and cough. Rapid breathing,auscultation wheezing, and whirring. He has been a heavy smoker for 30 years, smoking 2 packets of cigarettes a day.Arterial blood analysis gave the following values: PCO2 : 65 mmHg and HCO3 : 30 mmol/L. Calculate the pH of theblood (pKa=6.1 and a=0.03 mmol/L/mmHg)What is the underlying disorder?3/4:::

A buffer is a solution that can hold the pH of the solution at a certain value when small amount of…

Answered: 2. A 55-year-old patient was admitted…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 107E: A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C...

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A student is asked to bubble enough ammonia gas through water to make 4.00 L of an aqueous ammonia solution with a pH of 11.55. What volume of ammonia gas at 25C and 1.00 atm pressure is necessary?
Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
The pH of Mixtures of Acid, Base, and Salt Solutions a When 0.10 mol of the ionic solid NaX, where X is an unknown anion, is dissolved in enough water to make 1.0 L of solution, the pH of the solution is 9.12. When 0.10 mol of the ionic solid ACl, where A is an unknown cation, is dissolved in enough water to make 1.0 L of solution, the pH of the solution is 7.00. What would be the pH of 1.0 L of solution that contained 0.10 mol of AX? Be sure to document how you arrived at your answer. b In the AX solution prepared above, is there any OH present? If so, compare the [OH] in the solution to the [H3O+]. c From the information presented in part a, calculate Kb for the X(aq) anion and Ka for the conjugate acid of X(aq). d To 1.0 L of solution that contains 0.10 mol of AX, you add 0.025 mol of HCl. How will the pH of this solution compare to that of the solution that contained only NaX? Use chemical reactions as part of your explanation; you do not need to solve for a numerical answer. e Another 1.0 L sample of solution is prepared by mixing 0.10 mol of AX and 0.10 mol of HCl. The pH of the resulting solution is found to be 3.12. Explain why the pH of this solution is 3.12. f Finally, consider a different 1.0-L sample of solution that contains 0.10 mol of AX and 0.1 mol of NaOH. The pH of this solution is found to be 13.00. Explain why the pH of this solution is 13.00. g Some students mistakenly think that a solution that contains 0.10 mol of AX and 0.10 mol of HCl should have a pH of 1.00. Can you come up with a reason why students have this misconception? Write an approach that you would use to help these students understand what they are doing wrong.
Papaverine hydrochloride (abbreviated papH+Cl; molar mass = 378.85 g/mol) is a drug that belongs to a group of medicines called vasodilators, which cause blood vessels to expand, thereby increasing blood flow. This drug is the conjugate acid of the weak base papaverine (abbreviated pap; Kb = 8.33 109 at 35.0C). Calculate the pH of a 30.0-mg/mL aqueous dose of papH+Cl prepared at 35.0C. Kw at 35.0C is 2.1 1014.
The pH of a household cleaning solution is 11.50. This cleanser is an aqueous solution of ammonia with a density of 1.00 g/mL. What is the mass percentage of ammonia in the solution?
1. a. The surface of Venus is quite inhospitable with an average temperature of 450 ̊C and a pressure of 92 atm (earth). Under these delightful conditions, the pKw of water is estimated to be 24. What is the pH of neutral water on Venus? b. An aqueous acetic acid (HOAc) solution is 1.00 % dissociated. What will the concentration of H3O+ be if 0.82 g of sodium acetate (NaO2C2H3) is added to 100.mL of solution?
Atmospheric CO2 levels have risen by nearly 20% over thepast 40 years from 320 ppm to 400 ppm. (a) Given that theaverage pH of clean, unpolluted rain today is 5.4, determinethe pH of unpolluted rain 40 years ago. Assume thatcarbonic acid (H2CO3) formed by the reaction of CO2 andwater is the only factor influencing pH.CO2(g) + H2O(l) ⇌ H2CO3(aq)(b) What volume of CO2 at 25 °C and 1.0 atm is dissolvedin a 20.0-L bucket of today’s rainwater?
the pH of modern rain water (= 5.61) in equilibrium with air at 25°C and a total pressure of 1 atmosphere, with a partial pressure of CO2 (PCO2) = 10-3.4 atmospheres (which equals 400 ppm by volume). The Intergovernmental Panel on Climate Change (IPCC) estimates that CO2 concentrations in 2050 may reach 600 ppm (PCO2 = 10–3.22 atmospheres). (a) Calculate the pH of rain water in equilibrium with 600 ppm of CO2. (b) By what factor (i.e. multiplier) is (H+) higher or lower in 2050 rain water vs. modern rain water? Please answer very soon will give rating surely All questions answers needed
Farmers who raise cotton once used atsemic acid, H3AsO4, as a defikuabt at harvest time. Arsenic acid is a polyprotic acid with K1 = 2.5 x 10 -4, K2 = 5.6 x 10-8, and K3 = 3 x 10-13. What is the pH of a 0.500 M solution of arsenic acid?
Like any equilibrium constant, Kᵥᵥ changes with tempera-ture. (a) Given that autoionization is endothermic, how does Kᵥᵥ change with rising T? Explain with a reaction that includes heatas reactant or product. (b) In many medical applications, the value of Kᵥᵥ at 37°C (body temperature) may be more appropri-ate than the value at 25°C, 1.0X10⁻¹⁴. The pH of pure water at 37°C is 6.80. Calculate Kᵥᵥ, pOH, and [OH] at this temperature.
Three (3) transparent drinking cups or glasses capable of holding at least one (1) cup of fluid. One (1) measuring cup capable of holding at least one-cup of fluid. One (1) teaspoon-sized measuring spoon. One (1) tablespoon-sized measuring spoon. One and one-half (1.5) cups of hydrogen peroxide. Two (2) tablespoons of distilled water (bottled or tap water will also suffice and assume it has a pH of 7). Two (2) tablespoons of distilled white vinegar (acid). One (1) tablespoon of baking soda. One (1) teaspoon of liquid dishwashing soap. One (1) medium-sized baking potato (e.g. a Russet potato). One (1) kitchen knife (e.g. a chef’s knife). One (1) ruler that allows you to measure in centimeters and millimeters. One (1) pen/sharpie. One (1) small piece of paper or Post-it Note. Masking tape. Procedure: Using the sharpie and masking tape, label the three (3) drinking cups or glasses, identifying one drinking cup as “Acid”, another one as “Water”, and the remaining one as…

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