presented by Macmillan Learning Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K = 6.2 x 10-8, and K3 = 4.8 x 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO? (aq), which pK, value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 %3D O PK22 =7.21 O pK33 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO, (s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. = Hd Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Scier 7:13 PM 11/8/202 五 0 FZ F8 F10 F11 F12 PrtScr Insert Delete F4 F5 Backspace 23 7. 8. 3. 5. R. E D F H B. N W PgUp Alt Ctrl Home PgDn

presented by Macmillan Learning Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K = 6.2 x 10-8, and K3 = 4.8 x 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO? (aq), which pK, value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 %3D O PK22 =7.21 O pK33 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO, (s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. = Hd Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Scier 7:13 PM 11/8/202 五 0 FZ F8 F10 F11 F12 PrtScr Insert Delete F4 F5 Backspace 23 7. 8. 3. 5. R. E D F H B. N W PgUp Alt Ctrl Home PgDn

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...

See similar textbooks

Similar questions

1) Determine the pH during the titration of 74.5 mL of 0.348 M nitrous acid (Ka = 4.5×10-4) by 0.348 M NaOH at the following points. (a) Before the addition of any NaOH ? (b) After the addition of 18.0 mL of NaOH ? (c) At the half-equivalence point (the titration midpoint) ? (d) At the equivalence point ? (e) After the addition of 112 mL of NaOH ?
Design a buffer that has a pH of 6.70 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ką pKa HC,04 C,0,²- 6.4 x 10-5 4.19 H,PO4 HPO,2- 6.2 x 10-8 7.21 HCO3 co,?- 4.8 × 10-11| 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base =
In the titration of 25.0 mL of 0.1 M CH3COOH with 0.1 M NaOH, how is the pH calculated before the titrant is added? Group of answer choices The pH is based on the concentration of protons present in the solution, which is equal to the original concentration of the acid. The pH is calculated using the H-H equation for a buffer solution, using the ratio of the concentrations of the base and the acid, and the pKa of the acid. The pH is 7. The pH is calculated by determining the concentration of weak conjugate base present in the solution, using an ICE table to calculate the hydroxide ion concentration present after hydrolysis, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of excess hydroxide ions in the solution, subtracting pOH from 14, and taking the negative log of the result. The pH is calculated by determining the concentration of weak acid present in the solution, using an ICE table to calculate…
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH;*(aq) + Before (mol) Change (mol) After (mol) 5 RESET 0.200 0.100 +x 0.200 + x 0.200 - x -x 0.100 + x 0.100 - x 1.00 x 103 -1.00 x 10-3 2.00 x 10-3 -2.00 x 10-3 6.00 x 103 -6.00 x 10-3 7.00 x 10-3 -7.00 x 103 8.00 x 103 -8.00 x 103
The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 pK22 = 7.21 O pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO,(s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. pH = II
What is the pH of a solution when 100.0 mL of a 0.1M HCN solution (Ka =6.2 x 10 -10) is titrated with 55.0 mL of a 0.075 M NaOH solution? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ? . Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.
- Calculate the pH of a 1.00 L buffer solution containing 0.143 mol of acetic acid (HC₂H30₂) and 0.180 mol of sodium acetate (NaC₂H₂O₂). The Ka of acetic acid is 1.8 × 10-5. pH = Calculate the pH of the buffer solution after 0.0315 mol of HCl is added to the buffer. Assume the volume of the solution does not change. pH = Calculate the pH after 0.0315 mol of HCl is added to 1.00 L of pure water. pH =
A student needs to prepare a buffer solution with a pH of 4.18. Assuming a pKa of 4.69, how many mL of 0.1 M NaOH would need to be added to 15.0 mL of 0.1 M HB to prepare this buffer? Please include a proper (abbreviated) unit. HINT : Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pKa + log (Volume of OH minus/ (Volume of HB minus Volume of OH minus)
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
You start with 100.0 mL of 0.20 M CH3COOH in a flask. The Ka of CH3COOH is 1.8 x 10-5. You add 10.0 mL of 0.20 M NaOH. What is the pH of the solution after the NaOH is added? TRUE or FALSE: The solution produced by mixing the reagents in the question above is a buffer.
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 100.0 mL of the strong base has been added. The value of Ka for HC4H;O2 is 1.5 × 10-5 1 2 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC4H;O2(aq) + OH (aq) H20(1) + C4H,O2 (aq) Before (mol) |Change Imol) After | (mol) RESET 0.100 0.200 +x 0.100 + x 0.100 - x -x 0.200 + x 0.200 - x 2.00 x 103 -2.00 x 103 8.00 x 103 -8.00 х 10"3 1.00 x 102 -1.00 x 102 1.20 х 10"2 -1.20 x 102 2.00 x 10-2 -2.00 x 102