Please see screenshot for question 8. What is the PH of a solution with [H*]=1× 10-³M3]2HCNO|-3HF|None of the others9. What is the PH of a solution with [OH¯]=1x 10-ªM|10]9HF]11HCNO|None of the others10. What is [H*] in M for a solution with PH=1ANone of the others]1 × 10-6]1 x 10-10|1 × 10–1|1× 10-311. What is [H*] in M for a solution with POH=1]1 x 10–12|1 × 10-7|1 x 10-13x 10-9]None of the others12. Calculate the PH of a 0.01M HCl solution.]0.7B2.0В 171.4|None of the others

Hello. Since more than one question has been asked, the first question shall only be answered in…

8. What is the PH of a solution with [H*]=1 x 10-³M ]3 2HCNO ]-3HF |-2 ]None of the others 9. What is the PH of a solution with [OH ]=1 x 10-4M |10 ]9HF ]11HCNO ]None of the others 10. What is [H*] in M for a solution with PH=1 |None of the others B1x 10-10 ]1 × 10-6 ]1 × 10-1 1 x 10-3 11. What is [H*] in M for a solution with POH=1 |1 × 10-12 |1 × 10-7 ]1 × 10-13 |1 × 10-9 ]None of the others 12. Calculate the PH of a 0.01M HCl solution. A0.7 2.0 |1.7 |1.4 |None of the others

8. What is the PH of a solution with [H]=1 x 10-³M ]3 2HCNO ]-3HF |-2 ]None of the others 9. What is the PH of a solution with [OH ]=1 x 10-4M |10 ]9HF ]11HCNO ]None of the others 10. What is [H] in M for a solution with PH=1 |None of the others B1x 10-10 ]1 × 10-6 ]1 × 10-1 1 x 10-3 11. What is [H*] in M for a solution with POH=1 |1 × 10-12 |1 × 10-7 ]1 × 10-13 |1 × 10-9 ]None of the others 12. Calculate the PH of a 0.01M HCl solution. A0.7 2.0 |1.7 |1.4 |None of the others

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 32QRT

See similar textbooks

Similar questions

Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
The pH of 1.0 108 M hydrochloric acid is not 8.00. The correct pH can be calculated by considering the relationship between the molarities of the three principal ions in the solution (H+, Cl, and OH). These molarities can be calculated from algebraic equations that can be derived from the considerations given below. a. The solution is electrically neutral. b. The hydrochloric acid can be assumed to be 100% ionized. c. The product of the molarities of the hydronium ions and the hydroxide ions must equal Kw. Calculate the pH of a 1.0 108-M HCl solution.
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
Calculate [OH], pOH, and pH for each of the following. a. 0.00040 M Ca(OH)2 b. a solution containing 25 g KOH per liter c. a solution containing 150.0 g NaOH per liter
Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
A 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?