Macmillan Learning pH = Calculate the pH of a solution containing 0.0368 M glutaric acid and 0.024 M potassium hydrogen glutarate. The K₂ values for glutaric acid are 4.52 x 10-5 (K1) and 3.78 x 10-6 (Ka2).
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A: Answer shown in attachment provide in explanation box Explanation:
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A:
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- Calculate the pH of a solution containing 0.0396 M malic acid and 0.023 M potassium hydrogen malate. The Ka values for malic acid are 3.48 x 10-4 (Kal) and 8.00 x 10-6 (K₁2). pH =Calculate the pH at 25 °C of a 0.38M solution of trimethylammonium chloride pk of 4.19. Round your answer to 1 decimal place. pH = X Ś ((CH3),NHCI). Note that trimethylamine ((CH3)3 N is a weak base with aCalculate the pH of a 0.025 M solution of propanoic acid (Ka = 1.3 x 10-5). The answer is 1.6
- Given that pK₂ = 3.14 at 25 °C for HNO₂, what is the pH of 0.165 mol L-1 NaNO₂(aq) at 25 °C? What is the equilibrium concentration of HNO₂? pH = Number (Give your answer accurate to 2 decimal places.) Number mol L-¹ (Give your answer accurate to 2 signficant [HNO₂]eq figures.) =Neuramidic acid (HNad, pKa=8.0) is dissolved in an aqueous solution, and the pH is 6.0. What is the ratio of HNad to Nad-? Express as a ratio of x:1, where x is a whole number with no decimal point or decimal places, for example, 1:1 or 5:1 or 27:1. (No spaces.)Consider the equilibration of a weak base B (K₁ = 5.57 x 10-5) between water (phase 1) and benzene (phase 2). Which expression represents D, the distribution ratio? B represents the unprotonated form of the base and BH+ represents the protonated form of the base. O [B] 2 [B]₁ [BH+]2 [B]₁ + [BH+]₁ [B]2 [B]₁ + [BH+]₁ O [BH+]2 [BH+]₁ D= Calculate D at pH 8.43 if Kp = 44.0. Which expression represents Kp, the distribution constant? B represents the unprotonated form of the base and BH represents the protonated form of the base. [B]2 [B]₁ [B]2 [B]₁ + [BH+]₁ [BH+]2 [B]₁ + [BH+]₁ [BH+]2 [BH+]₁ Will D be larger or smaller at pH 7.00 than at pH 8.43? omaller
- What is the pH of a 0.290 M solution of aniline (C6H5NH2, Kb = 4.3 x 10-10)?Calculate the pH at 25 °C of a 0.32M solution of trimethylammonium chloride ((CH3)2NHCI). Note that trimethylamine ((CH3)3N) is N is a weak base with a pK of 4.19. Round your answer to 1 decimal place. = 0 pH =What is the pH of 0.093 ?0.093 � butanoic acid, C3H7COOH? The Ka of butanoic acid is 1.5 x 10-5.
- Write the expresson for the dissociation constant, Ka for an aqueous solution of butanoic acid. CH3CH2CH2CO2H. Calculate the PH of a 0.01M aqueous butanoic acid given that Ka for butanoic acid is 1.5 x 10-5 .-3 Calculate the pH of a 3.6 x 10-M solution of H2SO4 (Ka, 1.2 x 10-2). pH =Use the modified H-H shown below to calculate the blood plasma pH under the following conditions: [HCO3-] = 0.022 M and pCO₂ = 46 mmHg. Provide your answer to two decimal places. Do not enter units. Dissociation Constant pH = 6.1 Bicarbonate (mmol/L) HCO 0.03 x PCO₂ CO₂ Solubility Constant CO₂ Partial Pressure (mmHg)
