Part A MISSED THIS? Read Section 18.2 (Pages 788 - 799) ; Watch KCV 18.2B, IWE 18.2. a solution that is 0.16 M in HCHO2 and 0.13 M in NaCHO2 (Ka(HCHO2) = 1.8 × 10-4) Use the Henderson-Hasselbalch equation to calculate the pH of each solution: Express your answer to two decimal places. pH = 3.52 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

Part A MISSED THIS? Read Section 18.2 (Pages 788 - 799) ; Watch KCV 18.2B, IWE 18.2. a solution that is 0.16 M in HCHO2 and 0.13 M in NaCHO2 (Ka(HCHO2) = 1.8 × 10-4) Use the Henderson-Hasselbalch equation to calculate the pH of each solution: Express your answer to two decimal places. pH = 3.52 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 74QAP: Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a)...

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
V A solution is prepared at 25 °C that is initially 0.27M in chloroacetic acid (HCH₂CICO₂), a weak acid with K=1.3 × 10-³, and 0.48M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. -3 pH = 1 X Ś
Which is the best solution to buffer at pH = 10.50? (A) A buffer solution containing 0.25 M H2CO3 and 0.45 M Na2CO3; (Ka (H2CO3) = 4.3 x 10–7) (B) A buffer solution containing 0.25 M NaHCO3 and 0.45 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (C) A buffer solution containing 0.12 M NaHCO3 and 0.22 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (D) A buffer solution containing 0.12 M NH4Cl and 2.2 M NH3; (Ka (NH4+) = 5.6 x 10–10)
3. A solution was prepared by adding 4.95 g sodium acetate (NaC;H;O2) to 250.0 mL of 0.150 M acetic acid (K = 1.75 x 10). Assume negligible volume change. a) What is the pH of the resulting solution? PH: pk2 + log CH3 02) moles saium 4.959 0.06 mol %3D 2cent %3D 82gmu H: -log (1.73x 10) + log 0.24 moles 2cete 250 x 0.15 IL :00375 1000me PH : 4 1.96 O.06 (N2 G Hs0): 0.24m 0.230 L O.0375 : CCHS COOH): 0 15 m Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to it. What is the pH of this new mixture? b)
Calculate the hydronium ion concentration for a buffer solution that is 2.0 M in maleic acid (H2M) and 1.5 M in potassium hydrogen malanate (KHM) (Ka1=1.20x10-2; Ka2=5.96x10-7). Verify all your assumptions.
A 5.50 g sample of a weak acid with Ka 1.3 x 101 -4 was combined with 5.20 mL of 6.00 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.15. Part A What is the molar mass of the weak acid? || ΑΣΦ M = 417.93 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining ? g/mol
From the following choose the most appropriate weak base (when added to its conjugate acid) for making a buffer with pH = 4.50 O (CH3)3N (K, = 6.4 x 105) %3D O CgH5NH2 (K = 3.9 x 1010) O C2H5NH2 (Kg = 5.6 x 104) O HONH2 (K, = 1.1x 108) %3D O NH3 (K5 - 1.8 x 10 5)
MISSED THIS? Watch KCV 17.4, IWE 17.7: Read Section 17.4. You can click on the Review link to access the section in your e Text Consider the titration of a 23.0-ml, sample of 0.110 M HC,H,0; (K, =1.8 x 10) with 0.130 M NAOH. Part A Determine the initial pH. Express your answer to two decimal places. Avanauie dIter reD 18 at 10:59an leak-Strong Titrations oblem 3 MISSED THIS? Watch KCV 17.4, IWE 17.7; Read Section 17.4. You can click on the Review link to access the section in your e Text. rail D Determine the volume of added base required to reach the equivalence point Consider the titration of a 23.0-mL sample of 0.110 M HC,H3Os (K, = 1.8 x 10-) with 0.130 M NaOH. Express your answer in milliliters to three significant figures. ? ml Submit Reguest Answer Part C Determine the pli at 6.00 mL of added base. Express your answer to two decimal places.
Q2.9 What would be the pH of a buffer that is composed of mh of 0.10 M CH3 CaoNa? and 125 92 mL of 0.10M CH3COOH known: Ka (CH3 COOH) = 1.81x10-5 write. your answer to 2 decimal places.
7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid. 8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)
A sample of nitric acid, HNO3 is titrated with NaOH. Which of the following would be the best indicator to use? O Thymol Blue (pH range= 1 - 2.5) O Methyl Orange (pH range= 3- 5) Alizarian yellow R (pH range= 10 - 12) Cannot be determined from the information given. O Bromthymol Blue (pH range= 6 - 7.5)
When 22.6 mL of 0.229 M hydrochloric acid (HCI) and 22.6 mL of 0.229 M ammonia (NH3) are combined, what will be the pH value of the mixture? (Kp of NH3 = 1.8 x 10°, Ka x Kp = Kw for conjugate acid-base); Please keep your answer to two decimal place X.Xx.