Calculate the pH of a blood plasma sample with a total CO, concentration of 25.7 mM and bicarbonate concentration of24.4 mM. The relevant pKa of carbonic acid is 6.1Enter the answer with three significant figurespH 6.077Hyperventilatingcan result in a decrease in CO, (g) concentration in the blood.How would this affect the pH of the extracellular fluid?The pH increasesThe pH does not change appreciablyThe pH decreases

Given,The total concentration of CO2 is 25.7 mM.The concentration of bicarbonate is 24.4 mM.The pKa…

Answered: Calculate the pH of a blood plasma…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.58QE

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To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should be measured (HCO3-+CO2), this was determined by acidifying the sample and measuring the volume of CO2 released. The concentration of H2CO3 was 28.5 mmol/L, the pH of the blood at 37 ℃ is 7.48 with a pka of 6.10, what is the concentration of HCO3- in mmol/L in the blood? a) 27.36b) 22.77c) 28.50d) 29.60
Human blood contains one buffer system based on phos-phate species and one on carbonate species. Assuming that blood has a normal pH of 7.4, what are the principal phosphateand carbonate species present? What is the ratio of the two phosphate species? (In the presence of the dissolved ions andother species in blood, Kₐ₁of H₃PO4=1.3X10⁻², Kaₐ₂=2.3X10⁻⁷, and Kₐ₃=6X10⁻¹²; Kₐ₁ of H₂CO₃=8X10⁻⁷ and Kₐ₂=1.6X10⁻¹⁰.)
Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is 6x10-5) and 2.6g NaC6H5COOH in H2O. How much (in g) of the component of the buffer should be added in the 1000mL buffer so that its pH will be 3?
Which among SnCl2, BaBr2, CH3COONa is the basic salt
What will be the pH of a solution when 200ml of 0.1M HEPES in the basic form and 100mL of 0.1 M HEPES in the acid form are mixed together? The pKa of HEPES is 7.55
If the pH of a buffer solution is equal to the pKa of the acidin the buffer, what does this tell you about the relative concentrationsof the acid and conjugate base forms of the buffercomponents?(a) The acid concentration must be zero. (b) The base concentrationmust be zero. (c) The acid and base concentrations must be equal. (d) The acid and base concentrations must be equal tothe Ka. (e) The base concentration must be 2.3 times as large asthe acid concentration.
2. You are studying an unusual enzyme that produces hydronium ions (H3O+) during the courseof the reaction.You wish to maintain pH = 8.5 for the enzyme-catalyzed reaction. Which weak acid will serveas the better 0.1 M buffer for the reaction: HEPPS with pKa = 8.0, or, AMPSO with pKa = 9.0?Justify your answer by describing how the buffer “resists” change in pH and the chemical logicof why you chose the buffer you did.
Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?
Calculate the pH of each of the following points by titrating 50 mL of 0.40M imidazole (pKa = 6.993) with 0.41M KOH. Base added volume according to the equivalence volume: 0, 10, 90, 100, 120% Tabulate and plot Vavs. pH of the previous titration in Excel.
Determination of Ksp value given concentration of Ca2+ is 7.72705 ppm, and pH =9.24, and chemical equations (some sort of derivation using these equations and above values is needed to calculate the Ksp value)
Potassium cyanide is a toxic substance, and the median lethal dose depends on the mass of the person or animal that ingests it. The median lethal dose of KCNKCN for a person weighing 215 lblb (97.5 kgkg ) is 8.84×10−3 molmol . What volume of a 0.0250 MM KCN KCN solution contains 8.84×10−3 molmol of KCNKCN? ------ Gastric acid pH can range from 1 to 4, and most of the acid is HClHCl. For a sample of stomach acid that is 4.42×10−3 MM in HClHCl, how many moles of HClHCl are in 10.5 mLmL of the stomach acid? Express the amount to three significant figures and include the appropriate units.
Consider the spectrophotometric pH measurement of seawater with the indicator thymol blue illustrated at the opening of this chapter. The blue form of the indicator In22 on page 202 has maximum absorbance at a wavelength of 596 nm (nanometers). The yellow form HIn2 has maximum absorbance at 435 nm. Measurements of absorbance at the two wavelengths allows us to find the ratio [In22]/[HIn2]. How would you use this measurement to find the pH?

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