You begin by mixing 200.0 mL of 0.750 M HCl with 100.0 mL of an unknown concentration of NaOH solution.  When you examine the solution, you discover that the acid has been fully neutralized. In the second step of your experiment, you add an excess of aqueous iron (III) nitrate to the solution left over from the first. You notice that 1.605 grams of precipitate has formed.  After adding the aqueous iron (iii) nitrate how many moles of the excess reactant is there?   Use dimensional analysis to find the What the concentration of the original NaOH solution is ?

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A: The solution is given below -

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A:

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A: Given : Molarity of NaOH = 0.475M

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Q: You begin by mixing 200.0 mL of 0.750 M HCl with 100.0 mL of an unknown concentration of NaOH…

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A: The concentration of barium hydroxide can be caluculated using the following formula:

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A:

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.