Study 3: Titration of a Weak Acid, pKa = 5, with a Strong Base 10.00 mL of 0.100 M HX with 0.100 M NaOH A. Write down the balanced chemical equation between the titrant and analyte. Be sure to include (aq). B. Give all the equilibrium constants for the reaction. C. Calculate the mmoles of the initial amount of HX. (moles = M x mL)
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Study 3: Titration of a Weak Acid, pKa = 5, with a Strong Base
10.00 mL of 0.100 M HX with 0.100 M NaOH
A. Write down the balanced chemical equation between the titrant and analyte. Be sure to include (aq).
B. Give all the equilibrium constants for the reaction.
C. Calculate the mmoles of the initial amount of HX. (moles = M x mL)
Step by step
Solved in 2 steps
- Consider the titration of 50.0 mL of 0.100 M acetic acid with 0.0900 M NaOH. For acetic acid, Ka = 1.8 x 10-5. %3D a) What is the initial pH? (Be able to write the reaction responsible for the initial pH!) b) Determine whether the pH at the equivalence point is >, <, or = 7.00. (Be able to write BOTH the titration reaction & the reaction that is responsible for the pH at the equivalence point!)Calculate the pH during the titration with NaOH after addition of: a. 50 mL of 0.1 mol L-1 NaOH to 50 mL of 0.1 mol L-1 CH3COOH (Ka = 1.75 x 10-5). b. Based on the table below, which indicator (A, B or C) is most appropriate to track this titration? c. Explain your answer to item "b".Consider the reaction of a 20.0 mL of 0.220 M CsH5NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.215 M CSOH. a) Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. b) What quantity in moles of CsHsNH+ would be present at the start of the titration? c) What quantity in moles of OH- would be present if 12.0 mL of OH- were added? d) What species would be left in the beaker after the reaction goes to completion?
- 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)6. For the following acid -base titration H2SO4 (aq) + NaOH(aq) ----> A. Write down a complete and balanced reaction B. Find the concentration of OH-, Na+ and SO4 (2-) ions after the addition of 10 ml of 0.05 H2So4 to 50 ml, 0.5 M NaOHIf a 300 mg sample of Sodium Bicarbonate (98% NaHCO3) is titrated with 0.922 N sulfuric acid, what volume of the acid should be required to produce an end point? Atomic Weights :Sodium - 22.99Oxygen - 15.999Hydrogen - 1.008Sulfur - 32.06 Enter numerical value only; round off to 4 decimal places
- A solution containing 100.00 mL of 0.1800 M acetic acid (Ka = 1.78 x 10-5) is being titrated with 0.3500 M NaOH. Calculate the pH and construct a titration curve. a. Initially b. After the addition of 10.00 mL of NaOHThe following results were obtained in the titration of an unknown monoprotic acid (Use data from table). Students identified the acid as benzoic. Copy VNaOH (no first raw), then pH(all values) into your Lab Report template. Use the data you obtained to fill in the table below. Concentration of NaOH used, M 1.164 x 10-1 Mass of unknown aid used, g 0.3840 1) Find: a) Equivalence point, mL. b) Half equivalence point, mL. c) pKa d) Ka e) pKa from literature f) Percent Error g) Number of moles of NaOH, mol. h) Number of moles of acid titrated, mol. i) Molar mass of acid g/mol. j) Molar mass of acid, g/mol from the literature k) Percent erroracetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an erlenmeyer, you titrate 50 mL of this acid with 0.103 M NaOH and the phenolphtalein indicator duplo. The volume of NaOH needed to reach the equivalence point in both experiments was 48.96 mL and 49.11 mL. a. Write down the equilibrium reaction of dissolving vinegar in water, then write down the equation that reflects the acidic equilibrium constant!b. Calculate the average volume of NaOH needed to reach the equivalence point!c. Calculate the acidity of the vinegar in this sample!d. Calculate the initial pH of the vinegar solution before titrating!e. Calculate the pH at the equivalence point
- 5. A 100.0-ml aliquot of 0.100 M diprotic acid H2A (pK1 - 4.00, pK2 - 8.00) was titrated with 1.00 M NaOH Highlight each stage in the titration and the equivalence point. Also, obtain the first derivative of the curve (that is ApH / Avolume). Use the excel file below as your reference.construct a theoretical curves for the titration of 25 ml of 0.1 n nh4Oh Hcl (pkb=4.74) a. Write the equilibrium reaction b.Ph before titrant is added c.pH after adding 10ml titrant, 20ml,24ml,25ml,26ml,and 30ml of titrant ( please make a seperate solution for each ml)Hello, I need help solving and understanding the following question: You decide to perform a titration using 15 mL of a 1.2 M NH3 as your analyte and 0.6 M HCl as your titrant. Assume a new 15 mL of analyte is used for each step, determine the pH when the following volumes of titrant are used. (Kb = 1.8 x 10-5) a. 0 mL titrant added b. 20 mL titrant added