Calculate the pH during the titration of 100.0 mL of 0.200 M HCl with 0.400 M NaOH. First what is the initial pH (before any NaOH is added)? Answer: 1.69
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- In titrating 40.0 mL of 0.10 M of HCI solution with 0.15 M of KOH solution, what would be the pH of the solution after the addition of 25.10 mL of KOH? Please fill in the space with a numerical value with two digits or two decimal places without units Answer:(Incorrect) 367 mL of a 0.64 M hydrochloric acid solution is added to 238 mL of a 0.1 M hydroiodic acid solution. Calculate the pOH of the resulting solution. 0.37 (Your answer) 0.13 0.43 13.63 (Correct answer) 13.87Given the data for the following separate titrations, calculate the molarity of the NaOH: mL HCI Molarity HCI mL NaOH Molarity NaOH (a) 40.0 (b) 20.5 (c) 28.9 0.746 M 43.5 0.321 M 0.387 M 32.7 14.7 i i i M M M
- Part A Review Constants I Periodic Table A 250.0 mL buffer solution initially contains 3.0x10-2 M of HCHO2 and 3.0×10-2 M of NaCHO2. In order to adjust the buffer pH to 4.10, should you add NaOH or HCl to the buffer mixture? NaOH HCI Submit Previous Answers Part B Correct What mass of the correct reagent should you add? Express your answer using two significant figures. m = ΕΠΙ ΑΣΦ Submit Request Answer ? gWhat volume of 0.85 M NaOH (in mL) is needed to reach the equivalence point in a titration of 83.0 mL of 0.90 M HCIO4? Your Answer: Answer unitsIf a buffer solution contains 2.1 M acetic acid and 2.7 M sodium acetate, what is the pH of the buffer if the K, of the acetic acid is 1.8 x 10-5. Round to 2 decimal places. Your Answer: Answer
- Given the data for the following separate titrations, calculate the molarity of the HCl: mL HCl Molarity HCl mL NaOH Molarity NaOH a) 40.9 ? M 40.1 0.725M b) 19.6 ? M 31.6 0.289M c) 25.9 ? M 17.2 0.455Mv Question Completion Status: QUESTION 13 Consider an acid-base titration in which the base is dispenssd from a burette into a flask containing an acid. If any drops of the base adhere to the inner walls of the flask, but do not ackially mix with the solution, the calculated acid concentration would be O the same as the actual value. O lower than the actual value. O higher than the actual value. O Need more information QUESTION 14 What is the BEST numerical value for the quantity of liquid in the graduated cylinder? Save A Click Save and Submit to save and submit. Click Save All Answers to save all answers.Calculate the pH at the following points on the titration curve where 50.00 mL of 0.10 M nitric acid is being titrated with 0.15 M NaOH . (0, 10, 25, 50, 75, 100,, 125% titrated) Please answer
- 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 solutionrequired to reach the equivalence point, and the concentration of each HCl solution. Calculate the concentration (in M) of the unknown NaOH solution in each case. NaOH Volume (mL) HCl Volume (mL) [HCl] (M)a. 5.00 mL 9.77 mL 0.1599 Mb. 15.00 mL 11.34 mL 0.1311 Mc. 10.00 mL 10.55 mL 0.0889 Md. 30.00 mL 36.18 mL 0.1021 MFour solutions of unknown HClHCl concentration are titrated with solutions of NaOHNaOH. The following table lists the volume of each unknown HClHCl solution, the volume of NaOHNaOH solution required to reach the equivalence point, and the concentration of each NaOHNaOH solution. HClHCl Volume (mL)(mL) NaOHNaOH Volume (mL)(mL) [NaOH][NaOH] (M)(M) 24.00 mLmL 23.44 mLmL 0.1201 MM 11.00 mLmL 20.22 mLmL 0.0952 MM 23.00 mLmL 11.88 mLmL 0.1128 MM 3.00 mLmL 5.88 mLmL 0.1325 MM 1. Calculate the concentration (in MM) of the unknown HClHCl solution in the first case. HClVolume (mL) NaOH Volume (mL) [NaOH](M) 24.00 mL 23.44 mL 0.1201 M 2. Calculate the concentration (in MM) of the unknown HClHCl solution in the second case. HCl Volume (mL) NaOH Volume (mL) [NaOH] (M) 11.00 mL 20.22 mL 0.0952 M 3. Calculate the concentration (in MM) of the unknown HClHCl solution in the third case. HCl Volume (mL) NaOH Volume (mL) [NaOH][NaOH] (M) 23.00 mL 11.88 mL 0.1128 M…1. ACID-BASE TITRATIONS Four solutions of unknown HCI concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCl 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 each case. HCI Volume (mL) NaOH Volume (mL) [NAOH] (M) (a) 25.00 mL 28.44 mL 0.1231 M (b) 15.00 mL 21.22 mL 0.0972 M (c) 20.00 mL 14.88 mL 0.1178 M (d) 5.00 mL 6.88 mL 0.1325 M