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The pH of an aqueous solution with [OH-] of 2.45×10-8 M is ……………….. and the solution is……………….
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- Addition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition of bromthymolblue to the same solution also leads to a yellow color.(a) Is the solution acidic, neutral, or basic? (b) What is therange (in whole numbers) of possible pH values for the solution?(c) Is there another indicator you could use to narrowthe range of possible pH values for the solution?Which of the following is true for the reaction of BF3 + HF HBF4? BF3 is the Lewis Base BF3 is the Arrhenius base BF3 donates an electron pair HF accepts an electron pair HF is the Lewis Base Suppose you have 0.6 M solution of acid HB. Suppose further that K, <« 1 for this acid. Wsich of the following statements is true? (<) indicates much less. [H") and (8) are exactly 0.3 M [H') and (B] are <« 0.6 M (H'] and (B') are approximately 0.6 M [H'] and (B1 are < 0.6 M [H"] and (B] are exactly O MWhen a 100 mg NaCH3COO is dissolved in 1.00 L pure water at 25 °C, the resulting solution's pH is?
- The value of K for NO2-+H3O+---> HNO2+H2O is?A 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 hpIf 0.0751 moles of NaOH is added to 1.00 liters of 0.180 M CH3COOH (acetic acid), what will the pH of the resulting solution be? Ka of that acid is 1.8x10-5
- 3) 4 7 8. 9. 10 11 12 13 A solution is prepared at 25 °C that is initially 0.44M in diethylamine ((C,H,),NH, a weak base with K,=1.3 × 10 °, and 0.072M in diethylammonium chloride ((C,H5), NH,CI). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = Submit Assignr CornueA solution of carbonate (pKa = 6.3, 10.3) contains 0.0100 mol HCO3- and 0.00500 mol CO32-. Calculate the pH at equilibrium.if 1L of 1M acetic acid is mixed with .25 mole of solid NaOH (assume no volume change), what will the pH be of the resulting solution (Ka= 1.8*10-5)
- 0.3728, 0.9319, 1.4910 and 1.8638 g aliquots of KCI were dissolved in 4 separate 250 ml samples of distilled water. Calculate [H3O*] and the pH for each of the resulting solutions.Like any equilibrium constant, Kw changes with temperature. (a) Given that autoionization is endothermic, how does Kw change with rising T ? Explain with a reaction that includes heat as reactant or product. (b) In many medical applications, the value of Kw at 37°C (body temperature) may be more appropriate than the value at 25°C, 1.0 x 10-14. The pH of pure water at 37°C is 6.80. Calculate Kw, pOH, and [OH-] at this temperature.28. A solution is obtained by mixing 10 ml of 0.2 N KOH solution with 30 ml of 0.1 N CH3COOH. The pH of the solution would be: (Given: pKa of CH3COOH = 4.75; log 2 = 0.30) (a) 5.301 (b) 5.05 (c) 4.699 (d) 4.398