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Practice Problem ATTEMPT
Determine (a)
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Chemistry
- tion will be acidic. Simila Practice Exercise Predict whether the following solutions will be acidic, basic, or nearly neutral: (a) LiClO,, (b) Na,PO4, (c) Bi(NO3)3, (d) NH,CN. Finally we note that some anions can act either as an acid or as a base. For example, the bicarbonate ion (HCO;) can ionize or undergo hydrolvsis nn follarrow_forwardWhat is the pH of a 0.25 M solution of H3PO4? Ka = 7.2 x 10-³ (A) 0.25 (B) 7.2 x 10-3 (C) 0.0018 (D) 0.042 (E) 1.37arrow_forwardCalculate the percent ionization of ascorbic acid (HC6H7O6) in solutions of each of the following concentrations (Ka = 8.0e-05.)(a) 0.114 M (b) 0.438 M (c) 0.869 Marrow_forward
- Chemistry practice questionarrow_forwardWhich of the following reactions go to completion? (Select all that apply.) O Autoionization of water Strong acid-strong base neutralization reaction O Strong base dissociation in water Weak acid dissociation in water O O Oarrow_forwardanswer pleasearrow_forward
- Please correct answer and don't use hand raiting and don't use Ai solutionarrow_forwardWhich of the following statements is/are true? (Select all that apply) OThe higher the concentration of OH in a solution, the lower the pH. OThe higher the concentration of OH in a solution, the lower the pOH. O An acidic solution has a pH of geater than 7. The concentration of H30* in pure water is 1.00 x 107 M. OA Bronsted acid is a proton donor in an acid-base reaction.arrow_forwardPractice chemistry questionarrow_forward
- EXERCISE II -11 1. A chemist,, Hishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine, CH,NH2, ánd its salt, CH;NH2, and its salt, CH3NH;CI. (a) What should be the ratio of base to salt to obtain a pH of 10.00? (b) If he makes the solution 0.05000 M CH3NH2, how many moles of methyl ammonium chloride should he add to get the desired pH ? Kp = 5.00 x 104 2. A buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D 3. What change in pH will occur when 0.050 mmol of HOAC (Ka= 1.78 x 10) is added to 100.0 mL of a buffer solution that is 0.1000 M HOAC and 0.1000 M NAOAC? Assume no change in volume.arrow_forwardPlease correct answer and don't use hand ratingarrow_forward10. Ammonia (NH3) has base dissociation constant (K) of 1.8 x 10-5. What is the concentration of an aqueous ammo- nia solution that has a pH of 11.68? (LO 16.11) (a) 0.28 M (b) 3.6 M 1.3 M (c) 9.0 x 10-3 M 711 ***arrow_forward
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