9. A 50.0 mL solution of acetic acid (CH3COOH) was titrated. In the process 35 mL of a 1.00 M NaOH standard were consumed. find the molarity of the acetic acid. If the density of the acetic acid solution is 1.08 g/mL, calculate the % acetic acid in the sample.                               CH3COOH + NaOH CH3COONa + H2O

Consider a titration where 0.215 M potassium hydroxide is added from a burette to 10.00 mL of hydrochloric acid in an Erlenmeyer flask under the burette. A few drops of phenolphthalein are added to the acid in the Erlenmeyer flask. Sketch what this titration setup looks like then clearly identify the standard solution (or the titrant) and the analyte.

Dr. Donwonree tried to determine the vitamin C content in apple juice which he bought at CheMarket. He measured out 50.0 mL of the juice and added the HCl, KI, and starch. Then he started the titration by adding KIO3 solution into the juice. The concentration of the KIO3 solution was 0.200 M and it took only 1.50 mL of KIO3 to reach the endpoint. How much vitamin C (mg) is contained in 1.00 L of this apple juice?

A solution is prepared by mixing 0.10 L of 0.12 M sodium chloride with 0.22 L of a 0.19 M MgCl₂ solution. ▼ Part A What volume of a 0.21 M silver nitrate solution is required to precipitate all the CI ion in the solution as AgCl? Express your answer using two significant figures. IVD ΑΣΦ A A V = Submit Request Answer ? Review | Constants | Periodic Table L

A series of iron standard solutions need to be made from a 40 ppm iron stock solution provided. For the first dilution, pipet 5.00 mL of the 40 ppm stock solution into a 100.00 mL volumetric flask and dilute to mark. What is the new concentration of the diluted solution?

Please do not round values until the end. The final answer should be in 3 significant figures. Thank you!

A student is asked to standardize a solution of barium hydroxide. He weighs out 0.929 g potassium hydrogen phthalate ( KHC8H404, treat this as a monoprotic acid). It requires 36.8 mL of barium hydroxide to reach the endpoint. A. What is the molarity of the barium hydroxide solution? M This barium hydroxide solution is then used to titrate an unknown solution of hydrobromic acid. B. If 28.5 mL of the barium hydroxide solution is required to neutralize 13.3 mL of hydrobromic acid, what is the molarity of the hydrobromic acid solution? M

A student is asked to standardize a solution of calcium hydroxide. He weighs out 0.952 g potassium hydrogen phthalate (KHC8H4O4, treat this as a monoprotic acid).It requires 35.7 mL of calcium hydroxide to reach the endpoint.A. What is the molarity of the calcium hydroxide solution?  This calcium hydroxide solution is then used to titrate an unknown solution of nitric acid.B. If 15.6 mL of the calcium hydroxide solution is required to neutralize 29.1 mL of nitric acid, what is the molarity of the nitric acid solution?

If 21 mL of 3.2 x 10–5 M magnesium chloride and 15 mL of 1.5 x 10–4 M sodium fluoride are mixed, what are the concentrations of magnesium ion, chloride ion, sodium ion, and fluoride ion after mixing? Some choices may be used more than once, and keep an extra sig fig.   Question 9 options:     chloride ion     sodium ion     magnesium ion     fluoride ion   1.   1.87 x 10–5 M 2.   3.73 x 10–5 M 3.   6.25 x 10–5 M 4.   1.25 x 10–4 M 5.   1.50 x 10–4 M 6.   3.20 x 10–5 M 7.   1.50 x 10–4 M Answer and Explain

2. A student titrates 30.50 mL of a 4.50 g/L monoprotic acid (HA) with 25.00 mL of 0.10 M NaOH solution. a. Determine the concentration of the monoprotic acid (the ratio of the acid to base is 1:1). Concentration (2) = 4.50 30.50mL b. Determine the molar mass of the acid. = 147.542 M=4-50 = 180 0.0025 3. Determine the K, for a monoprotic weak acid with a pH of 3.5 at half the equivalence point. Ka = 10-3.5 4. What color will the solution turn indicating that the equivalence point has been reached?