2. An old bottle of sulfuric acid is found in the lab. The concentration of this bottle is unknown and needs to be determined. To do this, a lab technician first prepares a base titrant using sodium hydroxide by dissolving 3.0g of solid sodium hydroxide to 500mL of water. This base is then slowly added to a sample of the unknown acid, using phenolphthalein as an indicator, until a colour change from clear to pale pink is observed. The data collected from this lab can be found below: Volume of acid used: 25.0mL Volume of base added: 17.9mL Using this data, determine the concentration of the sulfuric acid solution

2. An old bottle of sulfuric acid is found in the lab. The concentration of this bottle is unknown and needs to be determined. To do this, a lab technician first prepares a base titrant using sodium hydroxide by dissolving 3.0g of solid sodium hydroxide to 500mL of water. This base is then slowly added to a sample of the unknown acid, using phenolphthalein as an indicator, until a colour change from clear to pale pink is observed. The data collected from this lab can be found below: Volume of acid used: 25.0mL Volume of base added: 17.9mL Using this data, determine the concentration of the sulfuric acid solution

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 107AE: A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution...

See similar textbooks

Similar questions

Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
0.2 mL of 0.10M NaOH is needed to titrate an unknown acid with a volume of 10.15mL. The final concentration of the resulting titrated sample is 0.163. Kindly explain how that value was found.
An unknown student takes an unknown mass of an unknown weak monoprotic acid and dissolves it in an unknown amount of water. The unknown student then divides the aqueous solution into two equal volumes, titrates one volume to a phenolphthalein endpoint, and then adds the other volume to the titrated solution. The pH of the combined volumes turns out to be 4.67. The Ka of the weak acid is
kindly help me with this problem thank youu!!1 Use floating decimal in your solutions but express all final answers to four (4) decimal places and enclose them in a box.
A buffer system works to keep pH within a narrow range. Buffer systemsare critical in all living cells/tissues. If pH were to measurably shift in a cell,what category of biological molecules would be most impacted, andwhat term refers to the resulting loss of their functional shapes? A buffer is a substance that, when it ionizes in water, creates a buffersystem. The substance and one of its ions represent a weak acid and aweak base. These form a pH-controlled equilibrium. Based on thedefinitions of acid and base, if [H+] increases, which would combine withthe H+, preventing a pH shift? If [H+] decreases, whichwould release H+ to counter a pH change? Check the one characteristic below that is important in a buffer system. maintains a neutral pH prevents pH from dropping prevents pH from rising minimizes change in p