Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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At 25℃, the pH of a 0.1 M KNO3 solution is *
< 7
Can’t be determined, since data given is not sufficient
=7
>7
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- Be sure to answer all parts. Calculate the hydroxide ion concentrations of the following solutions at 25°C, given the pOH. (a) pOH= 8.89 x 10 M |-[_HO] (Enter your answer in scientific notation.) (b) рОН - 4.52 M -[ HO] < Prev 15 of 28arrow_forwardFOR THESE 4 GIVE ANSWER TO 2 DECIMAL PLACE IN REGULAR NOTAION: 1) Determine the pH of a 0.275 M KOH solution. 2) Determine the pH of a 0.150 M aniline solution (Kb = 4.3x10-10). 3) Determine the pH of a 0.125 M HCl solution. 4) Determine the pH of a 0.175 M Phenol solution (Ka = 1.3x10-10). There is also questions in the image posted! Will thumbs up!arrow_forwardA solution is prepared at 25 °C that Is initlally 0.43M in dimethylamine ((CH, NH, a weak base with K, =5.4x10, and 0.15M in dimethylammonlum -4 and 0.15M In dimethylammonium bromide ((CH,),NH,Br) ((CH,) NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. bгomide 2. pH Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privac hparrow_forward
- The base protonation constant K; of allantoin (C,H,N;0;NH,) is 9.12 x 10 -°. Calculate the pH of a 0.76 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = ?arrow_forwardThe H3O+ ion mole concentration of the following solution was measured at 25 °C. Find pH and pOH of each solution. (a) 1.5X10-5 mol/dm3(b) 1.5 mmol/dmarrow_forwardComplete the following table for a solution at 25°C. pH [H3O] Solution is (c) (select) |1.0 х 10-7 м (е) (select) <7 (a) (select) <1.0 × 10-7 M () (select) (d) (select) 1.0 × 10-7 M neutralarrow_forward
- Determine the pH of a solution that is 0.00339 M HCl and 0.0281 M HCIO₂. The K₂ of HCIO, is 1.1 x 10-². pH = =arrow_forwardIf 0.50 L 0.20 M HF solution is mixed with solution A to make a mixed solution with a total volume of 1.00 L. Kw = 1.00x10-14; Ka(HF) = 6.6x10-4 at T=298K. (a) If solution A is 0.50 L 0.20 M HNO3, calculate the pH of the mixed solution. Ka(HNO3) = 100 (b) If solution A is 0.50 L 0.20 M NH4CI, calculate the pH of the mixed solution. Ko(NH3) = 1.8×10-5 %3D (c) If solution A is 0.50 L 0.20 M HNO2, calculate the pH of the mixed solution. Ka(HNO2) = 5.1×104 Hint: First list an equation that shows electrical neutrality in the solution. Also, neglect the [H*] contribution from water. Then use [H*] and the equilibrium constant(s) to express the anion concentrations in the equation you obtained for electrical neutrality, and you will find there is single unknown [H*] in the equation.arrow_forwardThe pH of an aqueous solution of 0.157 M ammonium perchlorate, NH4CIO4 (aq), is This solution is Submit Answer Retry Entire Group 8 more group attempts remainingarrow_forward
- Please solve faster, im waiting answers and i need answers now, thanks for solving Best regardsarrow_forward11 4000ol Ho00o 404 F-000HO HOO0HO HOOovale IHO 10H |-000Hal HO00H HO00'HO HO %3D ased on the definition of Ka, drag the tiles to construct the expression for the given acid. 1. CH,COOH(aq) + H,0(1) = H,O*(aq) + CH,COO-(aq) Construct the expression for Ka for the weak acid, CH,COOH. Question 26 of 27arrow_forwardA weak base has a Kb of 4.29E-10. Calculate the pH of a 0.250M solution of the weak base. pH = *** assume the temperature is 25°C.arrow_forward
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