Calculate the concentration of C6H5NH3+ and Cl in a 0.220 M C6H5NH3 Cl solution. Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by a comma. ΜΕ ΑΣΦ ? M Your submission doesn't have the correct number of answers. Answers should be separated with a comma. No credit lost. Try again. Submit Previous Answers Request Answer ▾ Part B Calculate the concentration of C6H5NH2, H3O+, and OH in a 0.220 M CH, NH, Cl solution. (Kb (C6H5NH2) = 3.9 x 10-10.) Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by commas. ΜΕ ΑΣΦ [C6H5NH2], [H3O+].[OH]= Submit Request Answer ? M

Calculate the concentration of C6H5NH3+ and Cl in a 0.220 M C6H5NH3 Cl solution. Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by a comma. ΜΕ ΑΣΦ ? M Your submission doesn't have the correct number of answers. Answers should be separated with a comma. No credit lost. Try again. Submit Previous Answers Request Answer ▾ Part B Calculate the concentration of C6H5NH2, H3O+, and OH in a 0.220 M CH, NH, Cl solution. (Kb (C6H5NH2) = 3.9 x 10-10.) Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by commas. ΜΕ ΑΣΦ [C6H5NH2], [H3O+].[OH]= Submit Request Answer ? M

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part 1,2and3
5.00 ml of 7.35 M Fe(NO3)3 is combined with 1.00 mL of 0.50 M HCIO4 and 4.00 ml of 2.00 x 10-2 M KSCN. What is the concentration of Fe3+ in the solution after the other reactants are added? Enter your answer with two decimal places. Example: 1.32 Do not include units in your answer.
Please help me answer questions 1 and 2. (Questions attached below) 1. When you arrive at the lab, 2.0 M H2SO4(aq) and 2.0 M HC2H3O2(aq) will be present. Youwill need to dilute these solutions using beakers and graduated cylinders from your drawerand DI water.i. Calculate the volume of the 2.0 M HC2H3O2(aq) and DI water needed to create 50.0 mLof 1.05 M HC2H3O2(aq).ii. Calculate the volume of the 2.0 M H2SO4(aq) and DI water needed to create 50.0 mL of0.75 M H2SO4(aq). 2. A 48.33-mL sample of 0.150 M NaBr is titrated into 50.00 mL of 0.145 M AgNO3. Bothsolutions had the same initial and final temperatures. The reaction occurred in a calorimeterwith a known heat capacity and produced 1546.03 J of heat.i. Write a balanced equation that is occurring.ii. Determine the theoretical yield of the solid.iii. Calculate the enthalpy of the reaction (kJ/mole of precipitate).
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What mass of Fe(OH)3 will be obtained when 100. mL of 0.150 M FeCl3 is mixed with 200. mL of 0.176 M NaOH? Be sure your answer has the correct number of significant digits. g Fe(OH)3 x10 X Ś 000 18 Ar
Determine the volume of 0.240 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is:H2SO4(aq)+2KOH(aq)→H2SO4(aq)+2KOH(aq)→ K2SO4(aq)+2H2O(l) 25 mL of 0.240 M H2SO4 Express your answer using two significant figures.
The concentration of acetylsalicylic acid in the original solution is 7.28 x 10-3 M. If the volume of this solution is 250.00 mL, calculate the moles of acetylsalicylic acid in this solution.
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5.00 mL of 2.32 M Fe(NO3)3 is combined with 1.00 mL of 0.50 M HClO4 and 4.00 mL of 2.00 × 10–2 M KSCN. What is the concentration of Fe3+ in the solution after the other reactants are added? Enter your answer with two decimal places. Example: 1.32
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Calculate the mass in grams of NaF needed to prepare 0.50 L of 1.47 M NaF solution. Enter your answer with one decimal place. Do NOT include units.