2. You are given 10.00 ml of a solution of unknown acid. The pH of this solution is exactly 5.83. You determine that the concentration of the unknown acid was 0.1224 M. You also determined that the acid was monoprotic (HA). a. What is the K, of your unknown acid NG 2 Info b. What is the pk, of your unknown acid NG 2 Info

2. You are given 10.00 ml of a solution of unknown acid. The pH of this solution is exactly 5.83. You determine that the concentration of the unknown acid was 0.1224 M. You also determined that the acid was monoprotic (HA). a. What is the K, of your unknown acid NG 2 Info b. What is the pk, of your unknown acid NG 2 Info

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 3P

See similar textbooks

Similar questions

Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of acetic acid added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.
Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.
Weak Acid Titration The weak acid was dissolved in 100 ml of H2O Use the titration data to calculate the Molar Mass of the unknown acid and to find the two Ka values and Pka values. H2A(aq) + H2O(l) ↔ HA-(aq) + H3O+(aq) Ka1= [ HA-][ H3O+]/[ H2A] HA-(aq) + H2O(l) ↔ A2-(aq) + H3O+(aq) Ka2= [ A2-][ H3O+]/[ HA-] Concentration NaOH: .1 M Unknown weak acid weight: 1.036 g Equivalence points: 20 ml and 41.5 ml pH: 2.84 at 10 mL, 4.73 at 20 mL, 6.185 at 30.75 mL, and 10.41 at 41.50 mL
Based on the table below: 1). create a titration curve of pH vs. volume NaOH (graph in in Excel). Indicate on graph the location of each pKa (pka1, pKa2, pKaR) , first and second equivalence point and pI. Show all your calculations. 2). 1st derivative plot of ΔpH / Δvol NaOH an the y-axis and average vol NaOH on the x-axis (graph in Excel). Highlight (label) the equivalence points Table 1.2 - Titration of an unknown amino acid with NaOH Vol. NaOH (mL) pH Avg.Vol. NaOH (mL) pH / Vol NaOH 0.00 2.12 0.5 0.02 1.00 2.14 1.5 -0.02 2.00 2.12 2.5 0.13 3.00 2.25 3.5 0.07 4.00 2.32 4.5 0.06 5.00 2.38 5.5 0.06 6.00 2.44 6.5 0.07 7.00 2.51 7.5 0.1 8.00 2.61 8.5 0.11 9.00 2.72 9.5 0.08 10.00 2.80 10.5 0.29 11.00 3.09 11.5 0.44 12.00 3.53 12.5 1.17 13.00 4.70 13.5 0.51 14.00 5.21 14.5 0.29 15.00 5.50 15.5 0.18 16.00 5.68…
The pKa of a weak acid was determined by measuring the pH of a solution containing the weak acid at 0.30 M and its conjugate base at 0.30 M. The measured pH was 8.0. What is the pKa of the weak acid?
In my slide, there is a table summarizing the pKa values for different acids. (1) when ranking the acidity level (how strong the acids are), a low pKa means high acidity. Why is that? (2) Calculate the phosphoric acid solution pH when the ratio of [H2PO4-]/[H3PO4] is 0.8.
ANSWER THE FOLLOWING WITH A COMPLETE SOLUTION. Compute for the pKa of benzoic acid (Ka = 6.3 × 10-5). What is the Kb of ammonia if its pKb is 4.75? What is the [OH-] of a solution if its pH is 5.69? Identify the [H+] of a solution with a pOH of 11.41. Identify if it is neutral, acidic or basic. What is the pH of a buffer prepared with 0.51 M disodium phosphate and 1.1 M sodium acid phosphate? (pKa of sodium acid phosphate = 7.21) Compute the pH of a buffer containing 0.62 M boric acid (Ka = 5.90 × 10-10) and 0.45 M sodium borate.
Weak Acids dissociate according to the following equation: HA(aq) + H2O(L) ⇌ H3O+ (aq) + A-(aq) In a lab, a buffer solution is made that contains both a weak acid (HA) and its conjugate base (A-), with the following concentrations: [HA] = 0.120 M [A-] = 0.200 M If the weak acid has a pKa value of 6.444, what is the pH of this buffer solution? (Please provide your answer to 3 decimal places.)
please calculate the neutralization equivalent for each run for part II. and for part III, calculate the neutralization equivalent for malonic acid and maleic acid
The measured pH of a prepared salicylic acid solution was 1.88. Based on this information, answer the items below. (Ka = 1.06 x 10-3) Determine the initial concentration (mol / L) of the acid in solution [Answer;Ci=0.177 mol/L] . And Knowing that salicylic acid is a solid, determine what mass the analyst must have weighed of the reagent to prepare 0.5 liters of this solution. (molecular mass of salicylic acid 138.12 g mol/L) [Answer; m=12.22 g]
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…