Solution e 2. Are the aqueous solutions of following chemicals acidic, basic, or

Question

Solution e 2. Are the aqueous solutions of following chemicals acidic, basic, or neutral? (a) NH4NOs: (b) Na2O: (c) KNO2 (d) SO3 (e) NHCH3O2 (Ka(HC2H3O2) 1.8 x 105, Ka(NH)-1.8x 105): (a) Write down the stepwise dissociation of H2SO4 solution in its aqueous solution. (b) Calculate the pH of 1.00 x 103 MH2S04 solution. (c) Calculate the percent dissociation of HSO4.(Note: Ka> 1, Ka2 -1.2 x 102) 3. 2HOCI(g) Calculate the concentrations of all species at equilibrium if 0.100 mole of pure HOCI(8) is initially placed in a 2.00-L flask. 4. At 25 °C, K 0.090 for the reaction: H2O(g) + Ch0(g) Useful formulae Amount dissociated mot Initial concentration (mol/L L--X 10096 Percent Dissociation: The PH Scale: pH -logiolH'l

Explanation / Answer

2.sol:-

a) NH4NO3 is acidic solution , because NH4NO3 is a salt of strong acid i.e HNO3 and weak base i.e NH4OH.

NH4NO3 + H2O -----> NH4OH + HNO3

b) Na2O is basic solution , because Na2O in water gives a strong base NaOH.

c) KNO2 is basic solution , because in KNO2 is a salt of Strong base i.e KOH and weak acid i.e HNO2.

d) SO3 form acidic solution because in water it gives H2SO4 strong acid.

H2O + SO3 -------> H2SO4

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