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givi [52]
3 years ago
9

If it requires 48.3 milliliters of 0.55 molar nitric acid to neutralize 15.0 milliliters of barium hydroxide, solve for the mola

rity of the barium hydroxide solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 yields Ba(NO3)2 + H2O
Chemistry
2 answers:
Gemiola [76]3 years ago
8 0
First you have to moles so multiply .0483L X .55M= .026565 Multiply moles by mole ratio which is 1/2, so the moles becomes .013283 now molarity=moles/volume; divide .013283/.015L=.885533M significant figures and you final answer is 0.89M
madam [21]3 years ago
4 0

<u>Answer:</u> The molarity of barium hydroxide solution is 0.8855 M.

<u>Explanation:</u>

The balanced chemical equation for the reaction is given as:

Ba(OH)_2+2HNO_3\rightarrow Ba(NO_3)_2+2H_2O

To calculate the molarity for a neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is HNO_3

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is Ba(OH)_2

We are given:

n_1=1\\M_1=0.55M\\V_1=48.3mL\\n_2=2\\M_2=?M\\V_2=15mL

Putting values in above equation, we get:

1\times 0.55\times 48.3=2\times M_2\times 15\\\\M_2=0.8855M

Hence, the molarity of barium hydroxide solution is 0.8855 M.

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