In an experiment, 8.67 ml of a .87M acetic acid solution was titrated with .250 sodium hydroxide. Predict by calculating the volume of base that should be used?

We need 30.2 mL of NaOH

Explanation:

Step 1: Data given

Volume of acetic acid solution = 8.67 mL = 0.00867 L

Concentration of acetic acid solution = 0.87 M

Concentration of sodium hydroxide = 0.250 M

Step 2: The balanced equation

CH3COOH + NaOH → CH3COONa+ + H2O

Step 3: Calculate the volume of sodium hydroxide

b*Ca*Va = a*Cb*Vb

⇒with b = the coefficient of NaOH = 1

⇒with Ca = the concentration of CH3COOH = 0.87 M

⇒with Va = the volume of CH3COOH = 0.00867 L

⇒with a = the coefficient of CH3COOH = 1

⇒with Cb = the concentration of NaOH = 0.250 M

⇒with Vb = the volume of NaOH = TO BE DETERMINED

1 * 0.87 M * 0.00867 L = 1 *0.250 M * Vb

Vb = (0.87 M * 0.00867 L) / 0.250 M

Vb = 0.0302 L = 30.2 mL

We need 30.2 mL of NaOH

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

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