Answer:
The molarity of the HCl solution should be 4.04 M
Explanation:
Step 1: Data given
volume of HCl solution = 10.00 mL = 0.01 L
volume of a 1.6 M NaOH solution = 25.24 mL = 0.02524 L
Step 2: The balanced equation
HCl + NaOH → NaCL + H2O
Step 3: Calculate molarity of HCl
n1*C1*V1 = n2*C2*V2
Since the mole ratio for HCl and NaOH is 1:1 we can just write:
C1*V1 =C2*V2
⇒ with C1 : the molarity of HCl = TO BE DETERMINED
⇒ with V1 = the volume og HCl = 10 mL = 0.01 L
⇒ with C2 = The molarity of NaOH = 1.6 M
⇒ with V2 = volume of NaOH = 25.24 mL = 0.02524 L
C1 * 0.01 = 1.6 * 0.02524
C1 = (1.6*0.02524)/0.01
C1 = 4.04M
The molarity of the HCl solution should be 4.04 M
10.00 mL of 4.038 M HCl required 25.24 mL of 1.600 M NaOH to be neutralized.
Let's consider the following neutralization equation.
NaOH + HCl ⇒ NaCl + H₂O
A 10.00 mL (Va) sample of HCl requires 25.24 mL (Vb) of a 1.600 M (Cb) NaOH to be neutralized. Since the molar ratio of NaOH to HCl is 1:1, we can calculate the concentration of the acid (Ca) using the following expression.
[tex]Ca \times Va = Cb \times Vb\\\\Ca = \frac{Cb \times Vb}{Va} = \frac{1.600 M \times 25.24mL}{10.00mL} = 4.038 M[/tex]
10.00 mL of 4.038 M HCl required 25.24 mL of 1.600 M NaOH to be neutralized.
Learn more: https://brainly.com/question/23307058
