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ow.com/ilrn/ takeAssignment/takeCovalentActivity.do?locator assignment-take&takeAssi; Part ll Use the Refereaces to access important values if needed for this question. An aqueous solution of nitric acid is standardized by titration with a 0.132 M solution of barium hydroxide. If 10.2 mL. of base are required to neutralize 16.7 mL. of the acid, what is the molarity of the nitric acid solution? I nitric acid An error has been detected in your answer. Check for typos miscalculations etc. before submitting your answer. Submit AnswerRetry Entre Group 9 more group attempts remaining eq eq

Explanation / Answer

Ba(OH)2 (aq) + 2HNO3(aq) -----------> Ba(NO3)2 (aq) + 2H2O(l)

1 mole                 2 moles

Ba(OH)2                                                                 HNO3

M1   = 0.132M                                                        M2   =

V1   = 10.2ml                                                          V2 = 16.7ml

n1 =1                                                                     n2 = 2

                M1V1/n1       =    M2V2/n2

                 M2               = M1V1n2/V2n1

                                      = 0.132*10.2*2/16.7*1

                                      = 0.1612 M

molarity of HNO3   = 0.1612 M

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