Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH, CH,CO,H, pKą = 4.874).[A¯]pHpKa+ log -[HA]Answer BankUsing the equation to calculate the quotient [A¯]/[HA] at three different pH values.[A¯]pH = 4.232[HA][A¯]1pH= 4.874[НА][A¯]pH = 5.373[HA]||

The given pKa value for a propanoic acid solution is 4.874. Henderson-Hasselblach equation is given,…

Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH,CH, CO,H, pKa = 4.874). [A¯] pH pK. + log = [HA] Answer Bank Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A¯] pH = 4.232 [HA] [A^] [HA] 1 pH = 4.874 = [A¯] pH = 5.373 [НА]

Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH,CH, CO,H, pKa = 4.874). [A¯] pH pK. + log = [HA] Answer Bank Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A¯] pH = 4.232 [HA] [A^] [HA] 1 pH = 4.874 = [A¯] pH = 5.373 [НА]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH₂CH₂CO₂H, pKa [HA] pH = = 4.352 || pH = 4.874 Answer Bank [A] + log Using the equation to calculate the quotient [A¯]/[HA] at three different pH values. [A-] [HA] [A-] [HA] - o = pka pH = 4.874).
Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH, CH, CO, H, pK, = 4.874). + log Answer Bank pH pK [A] [HA] Using the equation to calculate the quotient [A /[HA] at three different pH values. [A ] [HA] pH = 4.373 [A] pH = 4.874 [HA] [A] [HA] pH = 5.186
2. Joey was tasked to ensure that an enzyme responsible for keeping his species from extinction remains biologically active. To do so, he needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt KYA Benzoic acid, C6H5COOH 6.25 x 105 NaCH₂COO MUH Boric acid, H3BO3 5.81 x 107 NaH₂BO TWO Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (KYA, MUH, or TWO) will Joey store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 1.75 M stock solution (pH 7.00) of the same buffer system needed to prepare 250 mL of a 0.550 M buffer pH 7.00. After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as…
Determine the quantity of sodium acetate (CH₂COONa) needed to create buffer solution at a particular pH. Do this by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the mass of starting material required. The value of Ka for CH₂COOH is 1.8 × 105. Complete Parts 1-3 before submitting your answer. NEXT > Sodium acetate (CH₂COONa) is added to an existing 500.0 mL solution of 0.200 M CH₂COOH to form a buffer with a pH equal to 5.000. Let x represent the concentration of CH₂COO in the water after the addition of CH₂COONa. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. CH₂COOH(aq) Initial (M) Change (M) Equilibrium (M) 1.0 × 10¹5 x + 1.0 x 10-5 1 0 -1.0 × 10.5 x-1.0 x 10-5 X 1.8 × 105 x + 1.8 x 10-5 + 0.200 2 H₂O(1) -1.8 × 10-5 x-1.8 x 10-5 5.00 x + 5.00 -5.00 3 H,O*(aq) x - 5.00 1.0 × 10¹⁹ x + 1.0 × 10-9 + CH₂COO (aq) RESET -1.0 × 10¹⁹ x-1.0 ×…
2. Phoebe was tasked to ensure that an enzyme responsible for keeping her species from extinction remains biologically active. To do so, she needs to store it in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt PAH Benzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COO SAD Boric acid, H3BO3 5.81 x 107 NaH₂BO3 DOH Hydrogen cyanide, HCN 6.20 X 10-10 NaCN A. In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme? In your solution sheet, show calculations and briefly explain to support your answer. B. Write the equilibrium reaction involved in the buffer system. Write your answer on your solution sheet C. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.
BUFFERS, HYDROLYSIS OF SALTS 1. A 0.0250 M Ca(X)2 has a pH of 8.049. Ca(X)2 is composed of a Ca2+ cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X)2 into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C. Calculate the K₁ or Kb of X. D. Given the following Ką values of different weak acids, determine the identity of X. Weak acids Ka HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH3COOH 1.80 x 10-5 HNO₂ 4.00 x 10-4 ts
A formic acid buffer is prepared with 0.010 M each of formic acid (HCOOH) and Sodium formate (NaCOOH). The Ka for formic acid is 1.8 x 10-4. What is the pH of the solution? What is the pH if 0.0020 M of solid sodium hydroxide (NaOH) is added to a liter of buffer? What would be the pH of the sodium hydroxide solution without the buffer? What would the pH have been after adding sodium hydroxide if the buffer concentrations had been 0.10 M instead of 0.010 M?
A buffered solution containing dissolved aniline, CH,NH,, and aniline hydrochloride, CH, NH, Cl, has a pH of 5.27. Determine the concentration of CH, NH in the solution if the concentration of CH, NH, is 0.275 M. The pK, of aniline is $ 9.13. [CH_NH] = = Calculate the change in pH of the solution, ApH, if 0.386 g NaOH is added to the buffer for a final volume of 1.35 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M
: pH Titration A student is titrating 150.0 mL of a 0.300 M solution of lactic acid (pka of lactic acid is 3.85) with a 0.250 M solution of NaOH. . NOTE: You can use the generic formula of HA for lactic acid and A- for the conjugate base. 3.1 added. Round your answer to 2 decimal places. Calculate the initial pH of the lactic acid solution, before any NaOH has been pH = 3.2 Calculate the pH of the acid solution after the chemist has added 100.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH = 3.3 Calculate the pH of the acid solution after the chemist has added 200.0 mL of the OH solution to it. Round your answer to 2 decimal places. 0.2500 M pH =
Results Table pH pOH [OH] mol/L 9.9 4.1 7.9x 10'5 1. Complete the ICE table to calculate the K for magnesium hydroxide. Remember that solids are NOT included in equilibrium constant expressions. Mg(OH)200 = Mg + 2 OH initial O mol/L O mol/L change +Smol /L +25 mol +Smol/L +25mol equilibrium Show your K,p calculation: Ksp = [Mg2]CO-)2 %3D = 2 5mol/L = 7.9x 10 5 mol/L 14 x 105 mol/L Ksp= 4x (14xlo COHJ 2. Write your K,, value here: 2.5x10-13 3. Using the literature value of the Kp, calculate the pH value that corresponds to this Kap value. Ksp = 5.61 x 1o 12
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp compound CuBr CaCO3 Cal₂ Does solubility change with pH? Oyes no yes no yes no pH = 7 highest solubility pH = 8 X pH = 9 S
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K, data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 10 pH = 9 pH = 7 yes Ba (он), no yes Ca Cl, no yes K Cl no O O