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- ssignment Score: 85.7% Lx Give Up? Resources E Feedback uestion 17 of 28 > Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral pH = 8.39 pH = 5.50 H*] = 1.0 x 10-7 pOH = 10,32 pOH = 5.34 H* = 3.5 x 1013 OH| = 9.0 x 10- pOH = 7.00 H*| = 5.0 x 10 JOH"| = 8.9 x 10 Answer Bank Incorrectnment Score: 77.9% Resources O Hint cion 17 of 28> Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral H* = 1.0 x 10-7 pH = 8.39 pOH = 7.00 Answer Bank H|= 5.0 x 10 H| = 35 x 10 POH = 5 34 POH= 10.32 JOH= 89 x 10- JOH = 90 x 10 pH = 5 50 & mUse: pH = -Log [H30*] %3D 1. Round answers to the tenths place: (show work) a) Find the pH of a solution with [H30*] = 2.7 x 10-9 moles/liter Is this solution acidic, basic(alkaline) or neutral? b) Find the pH of a solution with [H30*] = 7.8 × 10~³ moles/liter Is this solution acidic, basic(alkaline) or neutral?
- Ihave some acetic acid that dissociates in water. [CH3COOH] = 0.405 M and [CH3COO]=0.505 M. K3=1.8x10-5. Find the pH=? (3 sig fig)a. What is the percent ionization in 0.80 M NH3 (Kb Percent ionization = % % = % 1.8 × 10-5)? b. What is the percent ionization in 0.090 M NH3 (Kb Percent ionization = c. What is the percent ionization in 1.0 M CH3NH₂ (Kb = 4.38 × 10¯4)? Percent ionization = = 1.8 × 10-5)?Macmillan Learning Calculate the hydronium ion concentration, [H₂O*], for a solution with a pH of 9.61. [H₂O+] = ****** C 4 R F V -0.983 Incorrect % G Search or type URL 5 T G B tv 6 MacBook Pro Y H & 7 N U J * 00 M 8 M I ( - 9 K < O V- H -O B P ' - : ; P { + 11 [ = 21 ? 11 1
- What is the ratio of NH4+ to NO2- in O2-saturated water when the pH is 8.20 and the pE is 4.42? (Ecell = 0.895)Wed Mar 8 ilibrium arro... Question 3 of 16 > 1 Assignment Score: tan Learning pH = AA 2.3 Assessment - G... Incorrect 31.3% achieve.macmillanlearning.com Chempendix - S... QHow to distingui... Resources Ex Give Up? J If the K₂ of a monoprotic weak acid is 5.9 x 10-6, what is the pH of a 0.21 M solution of this acid? S If the K_a of Feedback1. 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
- 2) a) Find the pH of 0.2 M ammonia solution (pka-9.74). b) Find the initial concentration of the HNO2 solution giving pH= 4.336 (K₁=1.58*10-¹0).B E 1. CH₂MgBr 2.HO 1. Na(CN)BH, pH 4-5 2.H₂O CHÍNH, NAOH 1. CH CH2NH2, Na(CN)BH, pH 4-5 2. Neutralizing work-up DoneTEFULL 5 80 Ⓒ Macmillan Learning For the diprotic weak acid H₂A, Kal = 3.4 x 10-6 and Ka2 = 7.8 x 10-⁹. What is the pH of a 0.0650 M solution of H₂A? pH = What are the equilibrium concentrations of H₂A and A²- in this solution? [H₂A] = [A²-] = 000 RFOO46 O O O O F % F5 MacBook Pro F6 & F7 F8 F9 F10 FIL + || M M F12