Carbonate (H2CO3/HCO3-) buffers are important in regulating the pH of blood at 7.40.  Note that the Ka for H2CO3 is 4.3 x 10-7. When a person exercises, muscle contractions produce lactic acid.  Moderate increases in lactic acid can be handled by the blood buffers without decreasing the pH of blood.  However, excessive amounts of lactic acid can overload the blood buffer system, resulting in a condition called acidosis if the blood pH falls to 7.35 or lower. Suppose a patient’s normal blood sample contains [H2CO3] = 0.0015 M and [HCO3-] = 0.0129 M.  If this patient exercises enough to produce 0.0010 mole of H3O+ per 1 L of blood due to production of lactic acid, would they be diagnosed with acidosis?

Q: Which of the following is/are true when CH3COOH is dissolved in water? I. At equilibrium, [CH3COOH]…

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Q: A 1.00 M solution of fluoroacetic acid is 10.0% dissociated in water at a certain temperature. The…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: An analytical chemest is titrating 150.6 ml. of a 0.6600 M solution of dhethylamine (C,H,) NH) wth a…

A: Answer: 1.73

Q: Calculate Ka from Equilibrium Concentrations At equilibrium a solution contains [HC2H3O2] = 0.0787 M…

A: Given,  At equilibrium a solution contains [HC2H3O2] = 0.0787 M and [H3O+] = [C2H3O2-] = 0.00118 M.

Q: b). What is the conjugate base of NH4? c) The Ka for NH4* is 5.5x10-10. What is the pKa for its…

A: b) Conjugate base is formed when a species releases a proton (H+).NH4+ →−H+ NH3so, conjugate base of…

Q: What is the pH of a buffer solution

A: Given :-   [C6H5OH] = 0.27 M  [C6H5O]- = 0.12 M  Ka = 1.0x 10-10 To calculate :- pH of the solution

Q: MISSED THIS? Read Section 18.2 (Page); Watch KCV 18.2A. A buffer is 0.100 M in NaC2H302 and 0.100 M…

A: The objective of the question is to identify which component of the buffer solution will neutralize…

Q: a. [CH3 COOH] = 0.85 M, [CH;CO0-] = 0.45 M (the pK, for acetic acid is 4.74) pH = b. [Н,РО, ] 3 0.50…

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Q: What [H2C03] needs to be added to 0.0250M NaHCO3 to obtain a buffer solution with a pH of 7.0?

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: 1. how many moles of KCN, are required to prepare 250.0mL of a solution with a pOH equal to 2.86

A: 1) pH of a salt formed from weak acid and strong base is pH = 7 + 1/2 ( pKa + log C ) pKa = - log Ka…

Q: A 0.13 M solution of a weak acid HA dissociates such that 95.2% of the weak acid remains intact…

A: A weak acid ionizes partially to produce the H+ ions in an aqueous solution.

Q: s this a buffer system? NaF + Ca5 (PO4)3OHCa5(PO4)3F + Na+ + OH-

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Q: A buffer solution contains dissolved C₆H₅NH₂ and C₆H₅NH₃Cl. The initial concentration of C₆H₅NH₂ is…

A: A solution which is a mixture of weak acid and its conjugate base is known as buffer. For…

Q: Healthy blood has a pH of 7.4. Estimate the ratio of [CO2] to [HCO3-] in the blood. Use the…

A: The dissociation of an acid (HA) in water can be represented as follows-The expression for acid…

Q: Part B How many grams of dry NH,CI need to be added to 2.00 L of a 0.100 M solution of ammonia, NH3.…

A:

Q: ou start with a solution of 0.8mol of acetic acid and then add 0.2mol of NaOH. What is the pH of the…

A: pKa of CH3COOH = 4.8moles of acetic acid = 0.8 molMoles of Determine the pH of new solution.

Q: Which one of the following compounds produces 3 mole IONS by dissociation when 1 mole of compound is…

A: When 1 mole of molecule is put into water then it will break into ions as the number of moles of…

Q: If the intrinsic solubility of an acidic drug is 20 mM and its pKa is 6, what is the lowest/highest…

A: Given data:The intrinsic solubility of an acidic drug = 20 mMpKa value for the acidic drug =6The…

Q: Which of the following compounds could be used to create a buffer with a pH of 9.00? ammonia, Kb =…

A:

Q: Determine the compound that is expected to be more soluble in acidic solution than in neutral or…

A: Answer :   FeCO3

Q: How many moles of NaOH must be added to 1.0 L of 2.0 M HC2H302 (Acetic Acid, Ka = 1.8x10^-5) to…

A: Buffer is solution which have tendency to resist pH change when small amount of strong acid or…

Q: Concentration Measured Theoretical pH Calculated Ka of acetic Literature Ka of of acetic acid, pH…

A: Average is found out  as:-                                  The sum of all the values/ the total…

Q: A buffered solution containing dissolved aniline, CH,NH,, and aniline hydrochloride, CH, NH, Cl, has…

A: The objective of the question is to determine the concentration of aniline in the solution and to…

Q: Determine the quantity of sodium acetate (CH3COONa) needed to create buffer solution at a particular…

A:

Q: You have 0.600 L of an 0.3 acetate buffer solution (i.e. [HC₂H3O2] + [C₂H30₂] = 0.300 M) at pH 5.30.…

A: Given: Volume of acetate buffer = 0.600 LMolarity of acetate buffer = 0.300 MHC2H3O2+C2H3O2- = 0.3…

Q: 0.20 moles of CuSO4 are added to 1L of NH3 1.20M solution. Calculate the concentration of Cu2+ in…

A: Data given: Moles of copper sulfate = 0.20 mol Molar concentration of ammonia = 1.20 M Volume of…

Q: A buffered solution containing dissolved aniline, C. H₂NH₂, and aniline hydrochloride, C6H, NH, Cl,…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.  It…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.