Determine the pH of a solution when 26.2 mL of 0.030 M HNO, is mixed with 18.6 mL ofA. 0.0060 M NAOH.pH =%3DB. distilled water.pH =C. 0.0080 M HCI.pH =D. 0.072 M KOH.

Answered: Image /qna-images/answer/0264af0d-8c15-48c0-842f-8fb5e0b49ac0.jpg

Answered: Determine the pH of a solution when…

Determine the pH of a solution when 26.2 mL of 0.030 M HNO, is mixed with 18.6 mL of A. 0.0060 M NAOH. pH = B. distilled water. pH = C. 0.0080 M HCI. pH = D. 0.072 M KOH.

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...

See similar textbooks

Similar questions

6. A 0.225L solution of H2CO3 is neutralized by 0.0880L of a 1.22 M Fe(OH)3 solution. What is the concentration of the H2CO3 solution?
What is the correct chemical equation for the neutralization reaction between HNO3 and Ca(OH)2 O A. HNO3 + Ca(OH)2 --> CANO3 + H20 O B. HNO3 + Ca(OH)2 --> Ca(NO3)2+ H20 O C. 2HNO3 + Ca(OH)2 --> Ca(N03)2+ 2H20 O D. HNO3 + 20Ca(OH)2 --> 2CANO3 + H20
Calculate the concentration of HCO3 in an aqueous solution of 2.57x10-2 M carbonic acid, H₂CO3 (aq). [HCO3"] = Submit Answer M. Retry Entire Group 8 more group attempts remaining
At a certain temperature, chlorine gas and carbon monoxide react to form carbonyl chloride: Cl2(g) + 2 CO(g) 2 coC(g). When 3.0 x 10-3 M Cl2 is mixed with 0.030 M CO and 9.0 x 10-3 M COCI, the concentration of ccl decreases. Which statement below is true? а. Кс 100 c. Kc = 30 d. Kç > 30 e. Kç = 100 f. Kç < 100 Your answer is incorrect. The correct answer is: Kc < 30
A east.cengagenow.com al Chemistry I X OWLV2 | Online teaching and learning resource from Cengage (References) Use the References to access important values if needed for this question. An aqueous solution of hydroiodic acid is standardized by titration with a 0.160 M solution of calcium hydroxide. If 17.1 mL of base are required to neutralize 19.3 mL of the acid, what is the molarity of the hydroiodic acid solution? M hydroiodic acid Submit Answer Try Another Version 5 item attempts remaining Visited Cengage Learning | Cengage Technical Support
1. Calculate the H30* and OH- concentrations according to the given ph values. Solution pH [H,O'] [OH] Unboiled distilled water 9.02 Boiled distilled water 6.54 1.0 M NaCl solution 6.02 1.0 M NaHSO4 solution 0.73 1.0 M Na2CO3 solution 11.48
6. What is the molarity of the H,SO if a solution of 0.162 M NaOH is used to neutralize 25.0 mL of H,SO4. To reach the end point, a total of 32.8 mL of NaOH were used.
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?
Emma titrated 20.00 mL of an HCL(aq) solution that has an unknown concentration with 0.1240 M NaOH(aq). The equivalence point is reached after adding 25.46 mL of NaOH(aq). a. Write out the complete balanced equation for the reaction that occurs in this titration. b. How many moles of NaOH were added to the HCl solution? c. How many moles of HCl were in the original 20.00 mL solution? d. What was the concentration of HCl in the original 20.0 mL solution?
50.0 mL of 0.100 M hydrochloric acid moles of H+ is equal to 0.005 100.0 mL of 0.200 M nitric acid moles of H+ is equal to 0.02 500.0 mL of 0.0100 M barium hydroxide moles of OH- is equal to 0.01 200.0 mL of 0.100 M rubidium hydroxide moles of OH- is equal to 0.02 When it asks you calculated the four moles of the solutions, this is what they are referring to.
5. What volume of 0.550 M NaOH do you need to titrate 40.0 mL of 0.260 M H&PO4. R-0
2. Answer the following questions about the reaction shown below. 3 H2O2(aq) + CH3OH(aq) -> 5H20(1) + CO2(g) a. Is this reaction classified as combustion, acid-base or redox? Justify your answer. b. What observation would you expect to see in the lab when this chemical reaction takes place? c. If 100 mL of 0.50 M H2O, and 100 mL of 0.50 M CH3OH are combined... What is the limiting reactant? and How many grams of CO, will be produced?