If 100.0 mL of 1.00 M NaOH and 100.0 mL of 0.500 M H2SO4solutions are mixed, wha

Question

If 100.0 mL of 1.00 M NaOH and 100.0 mL of 0.500 M H2SO4solutions are mixed, what will the concentration of the resultingsolution be? please don't skip step and explain briefly If 100.0 mL of 1.00 M NaOH and 100.0 mL of 0.500 M H2SO4solutions are mixed, what will the concentration of the resultingsolution be? please don't skip step and explain briefly If 100.0 mL of 1.00 M NaOH and 100.0 mL of 0.500 M H2SO4solutions are mixed, what will the concentration of the resultingsolution be? please don't skip step and explain briefly

Explanation / Answer

Each OH- from NaOH reacts with 1 H+ from H2SO4 amount of OH-: 0.1 L*1M = 0.1 mol OH- amount of H+ 0.1L *2 H+/1H2SO4 *0.5 M = 0.1 mol H+ H+ + OH- = H2O, so completely neutralize THus, 0.1L*1M = 0.1 mol Na+ 0.1L*0.5 = 0.05 mol SO42- All in 100 + 100 mL = 200 mL [Na+] = 0.1 mol/0.2 L = 0.5 M [SO42-] = 0.05 mol/ 0.2 L = 0.025 M

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