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The weak acid HQ has a pKₐ of 4.89.(a) Calculate the [H3O⁺] of 3.5X10⁻² M HQ.(b) Calculate the [OH⁻] of 0.65 M HQ.
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- Calculate the pKa of the weak acid HA, given that a solution that is 0.357 in HA and 1.24 in A- has pH = 5.32.Provide your answer rounded to 2 decimal digits.Define pKa for a weak acid. What is the relationshipbetween the value of the pKa and the strength of theacid? Do the same for a weak base.Define concept of Acid Strength and pKa ?
- Give typed explanation not written Consider the following Ka values for phosphoric acid, H3PO4.Ka1 = 7.1 x 10-3Ka2 = 6.3 x 10-8Ka3 = 4.2 x 10-13a.) What is the pH of a 4.0 M solution of H3PO4? b.) Determine the effectiveness of H2PO4acting as a base by calculating its Kb. c.) What is the pH of a 4.0 M solution of Na3PO4 (not H3PO4)?Would you expect Fe2+ to be the stronger Lewis acid? Explain.By coincidence, the Ka of CH3CO2H and the Kb of NH3 are both 1.8 × 10-5. Write appropriate acid-base equilibrium reactions (do not include physical states in your answer) and use them to determine whether each of the following 1.00 M solutions is acidic, basic, or neutral:
- Calculate the pH of 1.1 M C3H7COOH(aq) given that its Ka = 1.5×10-5.Provide your answer in decimal notation rounded to 2 decimal digitsSince the pH of 0.1 M acetic acid solution is measured as 2.88, the Ka value of acetic acid Calculate the degree of ionizationA 0.015 M solution of hydrogen cyanate (HOCN) has a pH of 2.67. Calculate the hydrogen cyanate concentration, hydronium ion concentration, and cyanate ion concentration in the solution. Calculate the Ka and pKa for the acid.
- Give a clear handwritten answer... An aqueous solution of base has a concentration of 0.156 M (@ 25 °C). The conjugate acid of the base is known to have a Ka value of 6.32 x 10-6. What is the pH of the solution?Complete the sentence for a strong acid, the equilibrium constant Ka is A. So small that HA is not completely dissociated b. So large that HA is completely dissociates into H3O+ and A- c. Neutral1. Arrange the following in order of increasing pH of their corresponding solutions. a. CH3NH3Cl, NaCH3COO, RbBr b. K2C2O4, C2H5NH3Br, Ba(ClO4)2 2. Oleic acid (which can be denoted as HOL), is a weak acid. Considering its sodium salt, sodium oleate (NaOL), calculate the pKa of HOL given that a 0.100 M solution of NaOL has a pH of 9.01. (hint: Kw=Ka * Kb).