Find the pH of a solution 2.0 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Explain step by step as you set up the equation and what each element represents.
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Find the pH of a solution 2.0 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Explain step by step as you set up the equation and what each element represents.
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- Find the pH of a solution 1.6 M in ethylamine CH3CH2NH2. For CH3CH2NH2 Kb=5.6x10-4. Report your answer to two decimal places.Calculate the pH of a 0.0500M solution of phenylacetic acid, C6H5CH2COOH and 0.0200M with its salt, C6H5CH2COONa. Ka= 4.9 x 10^-5Diethylamine, (CH3CH2)2NH, has a Kb of 8.6 x 10-4. What is the pH of a 0.22 M solution of diethylammonium chloride, [(CH3CH2)2NH2]Cl? Your answer should be to two places past the decimal point. A 0.15 M solution of an unknown monoprotic acid has a pH of 4.88, calculate the Ka for this unknown acid. You should have two significant figures in your answer and your answer should be in the following format (i.e. 1.0e-3).
- The acid dissociation constant Ka of alloxanic acid HC4H3N2O5 is ×2.2410−7. Calculate the pH of a 1.2M solution of alloxanic acid. Round your answer to 1 decimal place.Solution of glucose (concentration 1g/L) is diluted 1 : 10 and then 1 : 5. What is its final concentration? The ionization constant of methylamine, CH3NH2, (Kb) is 4.2 x 10–4. Write the dissociation equation and ionization constant expression for a 50 mM of methylamine. Calculate [OH-] in M, pOH, pH and [H3O+] in M. Write the dissociation equation and ionization constant expression for a 1 M of acetic acid. Calculate [OH-] in M, pOH, pH and [H3O+] in M. (pKa= 4.74). Calculate [OH-] in M, pOH, pH and [H3O+] in M of a 0.005 M NaOH.If the pH value of an aqueous solution of trimethylamine [(CH3)3N] is 10.75, what should the molarity of this solution be? (CH3)3N + H2O ↔ (CH3)3NH+ + OH-, Kb = 6,3 × 10-5
- Calculate the pH of a 0.0261 M trimethylamine hydrochloride solution. Kb ((CH3)3N) = 6.4 × 10−5. Report your answer to TWO places past the decimal.n the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of diethylamine, (C2H5)2NH to be 12.177. Use the information she obtained to determine the Kb for this base. Kb(experiment) =Calculate the pH of a 0.020 M solution of phenylacetic acid, C6H5CH2COOH. What will be the pH if the solution is made 0.050 M with its sodium salt, C6H5CH2COONa? K = 4.9 x 10-5. Provide solution
- Given that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar ratio of conjugate base-to-acid: [CH3CO2–]/[CH3CO2H] = 10/1?Write the expresson for the dissociation constant, Ka for an aqueous solution of butanoic acid. CH3CH2CH2CO2H. Calculate the PH of a 0.01M aqueous butanoic acid given that Ka for butanoic acid is 1.5 x 10-5 .The pH of a 1.1M solution of 4-chlorobutanoic acid (HC4HO₂Cl) is measured to be 2.24. Calculate the acid dissociation constant K of 4-chlorobutanoic acid. Round your answer to 2 significant digits. a K = 0 a 0 x10
