Concentration = 0.1634 M
Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following...
Exercise 14.47 Review Part Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the concentration (in M) of the unknown HCl solution in the third case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 24.00 mL 13.88 mL 0.1178 M Express your answer using four significant figures....
Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Part BCalculate the concentration (in M) of the unknown HCl solution in the second case.
Exercise 14.48- Enhanced - with Feedback Four solutions of unknown NAOH concentration are titrated with solutions of HCL The following table lists the volume of each unknown NAOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. HCI (M) NAOH volume HCl volume (mL) (mL) 0.2099 8.00 8.97 11 14 0 1061 21.00 10 85 12.00 0.0889 35 18 29.00 0.1021 You may want to reference (Pages 494-497) Section 14.6...
Four solutions of unknown NaOH concentration are titrated with solutions of HCl. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. NaOH Volume (mL) HCl Volume (mL) [HCl] (M) 7.00 mL 9.17 mL 0.2099 M 18.00 mL 10.84 mL 0.1111 M 15.00 mL 10.75 mL 0.0489 M 26.00 mL 35.18 mL 0.1421 M Part A: Calculate the concentration (in M)...
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
Titrations 1. A 50.00-ml NaOH sample of unknown concentration was titrated with 0.1274 M HCI. if 33.61 mL of the HCl solution were required to neutralize the NaOH sample, what is the molarity of the NaOH sample? Show the steps in your calculation 2. A 25.00-ml HCl sample of unknown concentration was titrated with 0.5631 M Al(OH)3. If 37.62 mL of the Al(OH) solution were required to neutralize the HCl sample, what is the molarity of the HCl sample? (Assume Al(OH)3 is...
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
An unknown concentration of HCl is titrated using known KOH. What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are titrate a 25.0 mL sample of the acid? Final answer: 0.218 M HCI questions, each has 10 points. An unknown concentration of HCl is titrated using known KOH.
Suppose that 10.00 mL HCl of unknown concentration is neutralized by 20.00 mL of a 1.50 M NaOH solution. Determine the concentration of the HCl solution 1.50 M HCI 3.00 M HCI 0.0750 M HCI 0.150 M HCI
Question 31 20 pts A 25.55 ml. sample of an HCl solution with an unknown concentration was titrated to equivalence with 41.48 ml. of a 0.4228 M NaOH solution. What is the concentration of the HCl solution? 06864M 0.2604M 3.840 M 1457M