What is the concentration of a solution of hcl in which a 10.0 ml sample of acid required 50.0 ml of 0.150 m naoh for neutralization? what is the concentration of a solution of hcl in which a 10.0 ml sample of acid required 50.0 ml of 0.150 m naoh for neutralization? 0.600 m 0.0300 m 0.750 m 0.150 m 7.50 m

The answer is 0.75M HCl

Explanation:

To calculate the concentration of 10 ml of HCl that would be required to neutralize 50.0 mL of 0.150 M NaOH, we use the formula:

To calculate the concentration of 10 ml of HCl that would be required to neutralize 50.0 mL of 0.150 M NaOH, we use the formula:

C1V1 = C2V2

C1 = concentration of acid

C2 = concentration of base

V1 = volume of acid

V2 = volume of base

From the information supplied in the question:

concentration of acid (HCl) is the unknown

volume of acid (HCl) = 10ml

concentration of base (NaOH) = 0.15M

volume of base (NaOH) = 50ml

C1 x 10ml = 0.15M x 50ml

C1 x 10 = 7.5

divide both side by 10

C1 = 0.75M

concentration of acid (HCl) is 0.75M

i'm assuming that it's c.) red bank..