gerald_mcdonald Posted March 30, 2011 Share Posted March 30, 2011 What volume of 0.100 M sulfuric acid would be required to neutralise a solution containing 0.500 g of sodium hydroxide and 0.800 g of potassium hydroxide? Any help showing the step-by-step working out to the above problem would be appreciated! Link to comment Share on other sites More sharing options...
CaptainBlood Posted March 30, 2011 Share Posted March 30, 2011 (edited) any hydroxides are strong acids which dissociate completely in the solution so just figure out the exact molar equivalent of monoprotic acid to neutralize it or half molar eq of di protic acid like sulforic acid Edited March 30, 2011 by CaptainBlood Link to comment Share on other sites More sharing options...
gerald_mcdonald Posted March 30, 2011 Author Share Posted March 30, 2011 any hydroxides are strong acids which dissociate completely in the solution so just figure out the exact molar equivalent of monoprotic acid to neutralize it or half molar eq of di protic acid like sulforic acid Could you do it? I don't understand what you're saying. And aren't hydroxides strong bases not strong acids? Link to comment Share on other sites More sharing options...
CaptainBlood Posted March 30, 2011 Share Posted March 30, 2011 sorry, what i meant to say is hydroxides are strong bases and you need a molar equivalent of strong acids to neutralize the solution. So just figure out how many moles of base you got and then add half as many moles of sulforic acid. Sulforic acid is di protic which means it has two hydrogens so you need half as many moles of diprotic acid as you would monoprotic acid like hydrochloric acid. Link to comment Share on other sites More sharing options...
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