Which of the following O The capacity of a buffer increases with increasing (Acid) and (Base) Ohe pH of a buffer solution increases when it is diluted The pH of a buffer solution decreases when it is diluted O The pH of a buffer will be O when [Acid]-[Base)
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![Which of the following statements is True? Acid) means molar concentration of the acid)
O The capacity of a buffer increases with increasing (Acid) and (Base)
he pH of a buffer solution increases when it is diluted
The pH of a buffer solution decreases when it is diluted
The pH of a buffer will be O when [Acid]-[Base).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F281eba4c-e5ff-43df-abed-6eacccf753e0%2F629c0eb6-f7d0-4eb7-945b-79d0d0257912%2Fnbsm6bo_processed.jpeg&w=3840&q=75)
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- Which of the following is TRUE if pH is higher than the pka of the buffer? O [weak acid] approximately 0 O [conjugate base] = [weak acid] [conjugate base] > [weak acid] O [conjugate base] < [weak acid]Buffer systems can absorb hydrogen ions from the blood to increase pH into homeostatic range (pH: 7.35 to 7.45)During what condition would buffer systems do this?Which of the following combinations would be the best choice to buffer the pH of a solution at approximately 7? Ionization Constants for Aqueous Weak Acids at 25 °C Acid K. (pK,) Conjugate Base Hydrogen phthalate ion, Cg H4(CO2H)(CO2) Acetic acid, CH3 CO,H Acetate ion, CH; CO2- 1.8 x 10-5 (4.74) Weak Acid Phthalic acid, C6 H4 (CO,H)2 1.3 x 10-3 (2.89) Dihydrogen phosphate Hydrogen phosphate ion, H2 PO4 Hydrogen phosphate ion, HPO42 6.2 x 10-8 (7.21) ion, HPO,2- Phosphate ion, PO,* 3.6 x 10-13 (12.44) O Na, HPO4 and NagPO4 O NaH2 PO4 and NazHPO4 O H;PO4 and NaH2 PO4
- Choose the FALSE statement An indicator can be used to monitor a buffer range When pH equals PKa of weak acid, the buffer capacity is the greatest Polyprotic acids have multiple stoichiometric points in their titration curve At the mid-point of titration of weak acid by strong base, the pH of the solution -does not equal the pKa of the weak acid The moles of titrant equals moles of titrateDefine the following:- pH- Buffer- pKaIn your own words, explain the Mechanism of Buffer Action.
- How much of the enzyme proteinase k (solute) is required to make 250ml of a solution with a concentration of .01mg/ml? (Weight/volume ratio)The least efficient buffer mixture?If 4 mL of 1 M NaOH is added to 100 mL buffer, would it still be a usable buffer according to the conventions? Explain why or why not.
- Tris NaCl buffer is known as?The normal range of the sodium electrolyte in the body is 134 to 145 mEq/L. The term mEq is dependent on the charge of the ion. Since sodium is a +1 ion, 134 mEq/L is the same as 134 mmol/L. An ion that has a greater positive or negative charge; however, will have 1 mEq for each positive or negative charge of the ion for every 1 mmol. For example, for Ca+2, 2mEq/1mmol. If the standard range of Magnesium in the body is 0.70 to 0.95 mmol/L, convert this value into mEq/L for the Mg2+ ion. (Use dimensional analysis to figure this out)Calculate the volume of TAE buffer that you will need to prepare a 100ml solution of 1X strength if you only have a 50X concentrated solution available.