Complete the charge balance for an aqueous solution of phosphoric acid, H₂PO4. [H+] = [OH-]+ Select the correct structure of H₂PO4. HO-P-0 OH =P-O OH₂ O 01PIOH OH₂
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- Fill in the left side of this equilibrium constant equation for the reaction of diethylmethylamine (C3H13N), a weak base, with water. D= K, oloCalculate the pH at 25 °C of a 0.24M solution of sodium hypochlorite (NaClO). Note that hypochlorous acid (HCIO) is a weak acid with a pk of 7.50. Round your answer to 1 decimal place. pH =Predict the products of the following acid-base reaction. Identify and label the conjugate acid / base pairs. CO,2 + H,O –
- Calculate the pH of 0.400 M solution of ascorbic acid, HC6H;O6. (Ka of ascorbic acid = 6.80 x 105)Calculate pH of 0.050 M NaClO, given that the Ka for HClO is 3.0 ×10–8 pH= 5.46 pH= 8.53 pH= 10.11 pH= 12.27Consider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×10
- Calculate the pH of a 8.3 x 10-M solution of H2SO4 (K, = 1.2 x 10-2). pH =3. For the following Lewis acid-base reaction, identify the acid, the base, and the new covalent bond formed. 3NO2 (g) + H₂O (1) 2HNO3 (aq) + NO(g)For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
- Given the following: [H3O+] = 5.112 x 10-13, please calculate the pOH.(Note please use 3 sig. figs for your answer.)Reaction 1: NaOH(s) -> Na+(AQ) + OH-(AQ) Reaction two: Na+(AQ) + OH-(AQ) + H+(AQ) + -> H2O(I) + Na+(AQ) Assuming reaction 1 has a enthalpy of 59.12 KJ/mol and reaction 2 has a enthalpy of 46.06 kJ/mol Calculate the change in enthalpy for the reaction shown below NaOH(s) + H+(aq) -> H2O(I) + Na+(aq) Delta H = ?en in die volgende Give one reason why benzene can act as an acid in the following reaction. O Na NOH +] H20