Paracresol (CHROH) has a Ka- 5.5 x 1011. if 100.0 mL of a 0.5000 M aqueous paracresol solution is mixed with 100.0 ml of 0.5000 M aqueous sodium hydroxide, the resulting solution will have a pH OA-7 OB. <7 OC.>7 O D. Cannot be predicted from the information given
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- Consider a solution initially containing 0.30 M of CH3NH2 mixed with 0.50 M of CH3NH3Cl in water. What is the pH after the addition of 6.415 mL of 0.10 M NaOH to 19.41 mL of this solution? (Kb for CH3NH2 = 4.47 × 10–4) Express your answer using at least three significant figures. Do not use scientific notation.The weak acid HXO2 has a dissociation constant of Ka = 4.50 × 10-10. A lab worker prepares of 1.500 M solution of this weak acid. What is the pH of this solution? Provide answer to 3 significant figures and no scientific notation please.3 Alice's pH meter broke and will only report [OH−]. What is the pH of a solution with a measurement of 1.122 mM?
- Calculate the pH of 100.00mL of 0.15 M pyridine solution after 106.00 mL of HClO4 0.15 M have been added. Kb pyridine = 1.7x10-9 ( Please type answer note write by hend)Determine the pH of the following solutions, given that Ka (HF) = 6.8 x 10-4.Hint: 1. Diagnose the scenario (i.e. strong acid + weak base, etc.), 2. If buffer solution, make useof Henderson-Hasselback eqn and 3. If strong acid/base added to buffer, write out reaction withstrong acid or base on the left hand side, then calculate ICE change. a. 0.5 moles of NaF b. A solution with 0.5 moles HF (Ka = 6.8 x 10^-4) and 0.5 moles NaF, to which 0.1 moles HClis added.Example 2What is the pH of the solution that results when 0.093 g of Mg(OH)2 Ksp = 7.1 × 10–12 is mixed with(a) 75.0 mL of 0.0500 M HCl?(b) 100.0 mL of 0.0500 M HCl?(c) 15.0 mL of 0.0500 M HCl? (d) 30.0 mL of 0.0500 M MgCl2?
- Calculate the expected pH of a buffer prepared by dissolving 1.3 mols of acetic acid and 0.4 mols of sodium acetate in enough water to make 500 ml of solution. Ka of CH3COOH = 1.8 x 10-5 Report answer to 2 decimal places.Question 5 4.1 Calculate the pH of a solution obtained by mixing 500.00 mL of 0.10 M NH3 with 200.0 mL of 0.15 M HCl. [Kb = 1.8 ]. Calculate the theoretical pH of this buffer solution(25mL of 1.0 M HC2H3O2 and 25mL of 1.0 M NaC2H3O2). The actual pH of the buffer was 4.44, now compare it to the theoretical value you calculated Info given pH 4.44 Ka= 1.8X10-5
- Determine [H3O+] of a 0.210 MM solution of formic acid (Ka=1.8×10−4Ka=1.8×10−4). I got 0.01 M but that was wrong3 What is the pH of 500 mL of water after the addition of 1 mL of 2M NaOH? HINT: you cannot use H-H equation for this question, but use Kw=10-14= [H+]*[OH-] (and c1v1=c2v2) 12.7 0.004 11.6 2.4 What is the pH of a 1 L solution to which has been added 3 mL of 3 M boric acid and 2mL of 1 M sodium borate? (pK of boric acid is 9.24) 9.89 9.46 9.02 8.59 9.24Calculate the pH of a solution containing 14.68 g of mandelic acid (152 g/mol) and 20.59 g of sodium mandelate (174 g/mol) in 400 mL solution (Ka=3.88x10-4). Please type answer note write by hend.