2. suppose that 21.37 ml of naoh is needed to titrate 10.00 ml of 0.1450 m h2so4 solution.
(a) write a balanced reaction equation for the acid-base neutralization.
(b) calculate the molarity of naoh based on the results of this titration.

0.1357 M

Explanation:

(a) The balanced reaction is shown below as:

(b) Moles of can be calculated as:

Or,

Given :

For :

Molarity = 0.1450 M

Volume = 10.00 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 10×10⁻³ L

Thus, moles of :

Moles of  = 0.00145 moles

From the reaction,

1 mole of react with 2 moles of NaOH

0.00145 mole of react with 2*0.00145 mole of NaOH

Moles of NaOH = 0.0029 moles

Volume = 21.37 mL = 21.37×10⁻³ L

Molarity = Moles / Volume = 0.0029 /  21.37×10⁻³  M = 0.1357 M

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.