8. (3 points) A 45.00 mL aliquot of a carbonic acid solution is titrated with 41.82...
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
45.00 mL of a 0.250 M H2SO4 solution is titrated with 0.100 M NaOH. a. What is the chemical equation that describes this neutralization reaction? b. What is the volume in mL of NaOH required to reach the equivalence point? c. At the equivalence point, what are the sodium and sulfate ion concentrations? d. At the equivalence point, what are the pH and pOH
This question has multiple parts. Work all the parts to get the most points. A 50.00-mL aliquot of 0.1900 M NaOH is titrated with 0.1900 M HCl. Calculate the pH of the solution after the addition of (Use a spreadsheet to complete this question.) a 0.00 mL of acid pH = 10.00 mL of acid pH = 40.00 mL of acid pH = 45.00 mL of acid pH = 49.00 mL of acid pH = 50.00 mL of acid pH...
You titrated a 25.00 mL solution of 0.02 M oxalic acid with a freshly prepared solution of KMnO4. If it took 41.81 mL of this solution to reach the endpoint, what was the molarity of the KMnO4? 0.0119 is wrong +/- 3 sig figs.
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
A.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 5.00 mL of 0.0960 M KOH. What is the solution pH to the nearest hundredths place? pKa1 = 6.35 and pKa2 = 10.33. B.) A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated with 0.0960 M KOH. How many mL of titrant are required to reach the first equivalence point? C. )A 20.0 mL sample of 0.0600 M carbonic acid (H2CO3) is titrated...
A 50.00 mL aliquot of 0.1548 M benzoic acid is titrated with 0.1325 M sodium hydroxide. Find (a) V. (b) the initial pH, (c and d) the pH after 10.00 and 30.00 mL are added, (e) the pH at Vand (1) the pH at V. + 10.00 mL. Sketch the titration curve. You may use all usual "assumptions" for the pH calculations. Benzoic acid is a weak acid. Write the numeric answers here: Sketch the titration curve here: a. mL...
A 15 ml aliquot of 1.00 M phosphoric acid is titrated with sodium hydroxide using phenolphthalein as an indicator. If it takes 20.00 ml of sodium hydroxide to reach the endpoint, what is the molarity of the sodium hydroxide? Answer with appropriate significant digits. H3PO4 (aq) + NaOH (aq) --> H2O (l) + Na3PO4
If 27.7 mL of the barium hydroxide solution was needed to neutralize a 7.44 mL aliquot of the perchloric acid solution, what is the concentration of the acid? Question 63 of 65 > Attempt 1 A barium hydroxide solution is prepared by dissolving 2.97 g of Ba(OH), in water to make 73.4 mL of solution. What is the concentration of the solution in units of molarity? concentration: 0.24 M The barium hydroxide solution is used to titrate a perchloric acid...
QUESTION 3 A 0.06 M HCl solution is used to simulate the acid concentration of the stomach. How many liters of "stomach acid" react with a tablet containing 0.37 g of magnesium hydroxide (58.33 g/mol)? Round answer to two sig figs and do not include units QUESTION 4 A 16.9 ml solution is 0.318 M HCI. What is the concentration after 56.8 ml of water is added to the solution? Round answer to 3 decimal places and do not include...