Please help with the following three questions. 1- An unknown 0.0500 M metal nit

Question

Please help with the following three questions.

1- An unknown 0.0500 M metal nitrate solution is either cobalt(II) nitrate or iron(III) nitrate. Both react with NaOH to form insoluble metal hydroxides (see Eqs. 12 and 13 in your lab manual). 10.00 mL of the 0.0500 M metal nitrate solution is titrated with 0.100 M NaOH solution. It took 15.1 mL to reach the equivalence point. Calculate the moles of NaOH needed to completely precipitate the metal ions from solution.

2- Based on the information in Question above, calculate the number of moles of unknown metal ion solution used in the reaction.

3- 0.5 pts Calculate the ratio of moles of NaOH to moles of unknown metal nitrate solution.

Explanation / Answer

number of moles of Na OH= molarity * volume in litres

=> number of moles of NaOH= .1*.0151 =.00151 moles

similarly moles of unkown solution is .05*.01=.0005 moles

ratio of moles of NaOH to unknown metal nitarte solution is .00151:.0005 = 3 to 1

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