Question

B) How many milliliters of 2.50 M. H2S04 are needed to neutralize 75.0 g of NAOH?C) if 54.8 mL of BaCL2 solution is needed to precipitate all the sulfate in 554 mg sample of NA2S04 (forming BAS04) what is the normality of the solution?D) if 27.5 mL of 0.125 M HCl solution is needed to neutralize a solution of CA(OH)2 how many grams of CA(OH)2 must be in the solution?

Answer 1

The volume is 2666.38L

Step-by-step explanation

Given information

The concentration (Molarity ) of H2SO4 is 2.50 M

The mass of NaOH is 75.0g

To find the milliliters of 2.50M of H2SO4, follow the steps below

Step 1: Write a balanced equation for the reaction

`\text{ H}_2SO_(4(aq))+\text{ 2NaOH}_((aq))\rightarrow\text{ Na}_2SO_4\text{ + 2H}_2O_((l))`

From the above-balanced reaction, you will see that 1 mole of the acid reacts with 2 moles of the base to give 1 mole of the salt and 1 mole of water

Step 2: Find the mole of sodium hydroxide using the below formula

`Mole\text{ = }\frac{\text{ mass}}{\text{ molar mass}}`

Recall that, the molar mass of NaOH is 39.997 g/mol

`\begin{gathered} Mole\text{ = }\frac{75}{39.997\text{ }} \\ \text{ Mole = 1.875moles} \end{gathered}`

From the calculations, you will see that the mole of NaOH is 1.875 moles

Step 3: Calculate the mole of sulfuric acid using a stoichiometry ratiO

`\text{ H}_2SO_4\text{ + 2NaOH }\rightarrow\text{ Na}_2SO4\text{ + 2H}_2O`

1 mole of H2SO4 is equivalent to 2 moles of NaOH

Let x represent the number of moles of H2SO4

Mathematically,

`\begin{gathered} 1\text{ mole of H}_2SO_4\text{ }\rightarrow\text{ 2 moles of Hno3} \\ \text{x moles}\rightarrow\text{ 1.875 moles} \\ Cross\text{ muliply} \\ \text{ 1 }*\text{ 1.875 2}*\text{ x} \\ 1875\text{= 2x} \\ Divide\text{ both sides by 2} \\ (1.875)/(2)\text{ = }(2x)/(2) \\ x\text{ = 0.9376 mol} \end{gathered}`

Hence, the mole of H2SO4 is 0.9376 moles

Step 4: Find the volume of the solution using the below formula

`\text{n = c }*\text{ v}`

Where,

n = is the number of moles

C = concentration in molarity

V = Volume of the solution in Liters

`\begin{gathered} 0.9376\text{ = }(2.50)/(V) \\ cross\text{ multiply} \\ 0.9376* V\text{ = 2.50} \\ Divide\text{ both sides by 0.9376} \\ V\text{ = }(2.50)/(0.9375)\text{ = 2.666 L} \\ \\ Convert\text{ ml to l} \\ 2.666*\text{ 1000 = 2666.38 mL} \end{gathered}`