Calculate the pH of a solution that is 0.69 M HF and 1.00 M KF. Ka = 7.2 x 10-4 pH = Submit Answer Try Another Version 1 item attempt remaining
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Calculate the pH of a solution that is 0.69 M HF and 1.00 M KF.
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- 4. The pH of 1.50 mol/L acid is measured to be 5.75. For this acid, the Ka is 10-5.25 = [H₂₂0] A. 2.1 x 10-¹2 B. 1.8 x 10-6 C. 2.4 x 10-6 D. very large Chatz (H30] = 1.77x10-6 = 1,8x10-6 In the following information to answer the next question."uonsanh stm The hydroxide ion concentration of an aqueous solution of 0.532 M acetylsalicylic acid (aspirin), HC9H¬O4, is [OH]= M. Submit Answer Retry Entire Group 9 more group attempts remaining Next 10/2 prt sc delete home fg ho 144 num & backspace %3D lock Y hc 3: 00 近In lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and a 1.0 M NaOH solution. You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. What volume (mL) of the 1.8M acetic acid solution, NaOH solution, and deionized water should you combine? Show all work.
- Questions 30-35 refer to the same weak acid/strong base (WA/SB) titration. Prior to the beginning of the titration, there were 0.0090 moles of hypobromous acid present in the flask. The Ką of hypobromous acid is 2.8 x 10-9. (Q30) A 30.00 mL solution of 0.300 M hypobromous acid (HBRO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LIOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)?How many milliliters of water have to be added to 143.8 mL of 0.25 M HCI to reduce the concentration to 0.10 M HCI? Vwater = mL eTextbook and Media Hint Save for Later Attempts: 0 of 2 used Submit Ans O Type here to search 10 insert @ %23 $ & * 4 7 8. 10 %3D Q W R PI A G K C V B NM pause alt alt ctri1. Complete the reaction NaOH → Na+¹ + i 2. What is the pH of a 0.001000 M NaOH solution ? first, find the [H3O+¹] using Kw Kw [ [H3O+¹] = [ |] [ pH = -log( a. acetic c. phosphoric g. sulfurous n. HPO3-2 u. 0.2500 aa. 2.6990 gg. 5.000 x 10-12 mm. conjugate acid b. hydrochloric [] d. perchloric e. hydrofluoric 1. Mg+2 S. HS-1 t. S-2 z. 1x 10-14 x. 1.000 x 10-3 y. 3.0000 CC. 11.0000 dd. 2 ee. 1 ff. 2.000 x 10-³ ii. 0.01250 jj. 0.22100 kk. 0.05656 II. acid pp. conjugate base -2 i. OH-1 j. H30+1 k. SO4² there is complete ionization f. sulfuric h. hydrosulfuric -2 0. H₂PO3-1 p. CO3-² q. HCO3-1 r. H₂S v. 0.1000 w. 0.02500 bb. 1.000 x 10-11 hh. 11.3010 oo. base m. Cl-1
- (Incorrect) 51 mL of 0.060 M NaF is mixed with 17 mL of 0.15 M Sr(NO3)2. Calculate the concentration of F in the final solution. Assume volumes can be added. (Ksp for SrF₂ = 2.0×10-10) 0.0075 M (Your answer) 0.00012 M (Correct answer) 0.038 M 0.045 M 0.015 M1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/L3. Titration: Strong Acid / Weak Base. (I warned you to be ready!) Here's the cool chart! Analyte: 20.00 mL 0.100 M Hydrazine (N₂H4) Hd A: initial Vertical (Value) Axis Title 0 B: half equivalence C: equivalence 5 10 15 20 Titrant: mL of 0.100 M HCI added 25 20.00 mL of 0.100 M hydrazine (N₂H4, pKb = 5.77) is titrated with 0.100 M HCl. a) Find the initial pH (point A) and the pH at the equivalence point (point C). b) Find the pH at the half equivalence point (point B).
- - 144 / Natural Sciences / Chemistry And Polymer Science / Chemi zzes / Buffers en Titrasies | Buffers and Titrations A 0.386 g sample of propanoic acid (CH3CH,COOH, K, = 1.3. x 10-5) was dissolved to a final volume of 50.0 cm, This solution underwent titration with 0.32 M NaOH. Calculate the pH of solution at the equivalence point. %3D fi h- Bi ek Please give the answer to 2 decimal places. Ge pl Answer: Check3 Solid potassium fluoride is slowly added to 75.0 mL of a 0.233 M calcium bromide solution until the concentration of %. fluoride ion is 0.0632 M. The percent of calcium ion remaining in solution is Submit Answer 20 E $ 4 R F Use the References to access important values if needed for this question. Retry Entire Group % 5 Cengage Learning Cengage Technical Support T G ^ 6 6 more group attempts remaining B Y H ← & 7 U N * 00 8 J ▶ M ( 9 K O ) 0 L P Previous Email Instructor + 11 [ Next> Save and Exit 11 1 dt of a. What is the pH of a buffer solution that is 0.16 M NH, and 0.16 M NH₂+? K₁ for NH, is 1.8 x 10-5. pH = 9.3 b. What is the pH if 17 mL of 0.21 M hydrochloric acid is added to 555 mL of this buffer? pH = Submit Answer [References] Try Another Version 9 item attempts remaining