0.178 L of aqueous HCl solution of unknown concentration was titrated with 0.825 M KOH (aq). 68.4 mL of the base was used to reach the endpoint of the titration. What is the concentration (M) of the acid? OA, 3.2 M Ов. 0.453 М O. 0.215 M OD. 2.1 M O E. 0.317 M

A 50 mL solution of NaOH was titrated with 39.7 mL of 0.9781 M HCl. What is the concentration of the NaOH solution?

H2. Titrations are performed by a scientist in the laboratory as follows: a solution of deuterated hydrochloric acid contains 1.08 g DCl in 750 ml of deionised, distilled water. An average amount of 14.95 ml of the DCl(aq) solution is titrated with 25.0 ml of Ca(OH)2 to produce an endpoint (as determined by an appropriate indicator). What is the molarity of the Ca(OH)2 solution? You must include all of your calculations    Please give typed answer

A 30.00 ml sample of phosphoric acid is titrated with a 0.050 M magneisim hydroxide solution.  The initial buret reading is 4.71 mL; the final buret reading is 31.09 mL.  What is the concentration of the unknown phosphoric acid solution?     2.64 M     0.100 M     0.0293 M     0.0879 M     0.0310 M

By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M

I have 28.63 mL of an unknown-concentration Mg(OH)2 (aq) solution. I find that, when I add 23.33 mL of 0.1060 molar HCl(aq) to this solution, the acid and base exactly neutralize each other. What was the original concentration of the Mg(OH)2 solution? a. 3.151 molar O b. 0.1728 molar c. 0.04319 molar d. 0.06504 molar e. 0.08638 molar Clear my choice Previous page Z 3 $ 4 n 5 80 MacBook Pro 6 & 11 8 Next page

A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1886 M0.1886 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.42 mL12.42 mL of the standard solution. What is the concentration of the original sulfuric acid solution?

A 0.124 M NaOH(aq) solution was used to titrate 20.00 mL of an NH3(aq) solution that has an unknown concentration. The equivalence point is reached after adding 22.50 mL of HCl(aq).   a. Write out the complete balanced equation for the reaction that occurs in this titration. b. How many moles of HCl were added to the NH3 solution? c. How many moles of NH3 were in the original 20.00 mL solution? d. What was the concentration of NH3 in the original 20.0 mL solution?

A 25.0 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.105 M NaOH (aq). It took 68.8 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.

A 0.8159 g sample of HCl was placed into a 50 mL volumetric flask and the sample was thoroughly dissolved in water to make 50 mL of solution. It required 22.07 mL of NaOH to reach the endpoint in the titration. What is the molarity of the NaOH solution? I mg IHE/ 2.022 4 mol 0.81599 Hcl 36.4bg.