25 ml of a solution of barium hydroxide on titration with 0.1 molar solution of hydrochlroric acid gave a titre value of 35 ml . The molarity of sodium hydroxide is ?
You mean the molarity of the parent
We assess the following stoichiometric equation:
And thus 2 equiv acid are required to neutralize each equiv barium hydroxide.
And, thus, by the given stoichiometry, there was an initial concentration of .......
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The molarity of the barium hydroxide solution can be calculated using the following formula:
M1V1 = M2V2
Where: M1 = Molarity of barium hydroxide solution V1 = Volume of barium hydroxide solution used (25 mL = 0.025 L) M2 = Molarity of hydrochloric acid solution (0.1 M) V2 = Volume of hydrochloric acid solution used (35 mL = 0.035 L)
Plugging in the values:
M1 * 0.025 = 0.1 * 0.035
M1 = (0.1 * 0.035) / 0.025
M1 = 0.14 / 0.025
M1 = 5.6 M
So, the molarity of the barium hydroxide solution is 5.6 M.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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