34.62 ml of a 0.1510 m barium hydroxide solution was needed to neutralize 50.0 ml of a hydrochloric acidsolution. what is the concentration of the original hydrochloric acid solution?

0.104 M

Explanation:

For the titration of an acid and a base , the relation between the molarity and volume is as follows -

M₁V₁ = M₂V₂

where ,  

M₁ = concentration of acid ,  

V₁ = volume of acid ,

M₂ = concentration of base ,  

V₂ = Volume of base ,

from , the question ,  

M₁ = ?

V₁ = 50.0 mL

M₂ = 0.1510 M

V₂ = 34.62 mL

Using the above formula , the molarity of the stock solution , can be calculated as ,  

M₁V₁ = M₂V₂

M₁ * 50.0 mL  = 0.1510 M *  34.62 mL

M₁ = 0.1510 M *  34.62 mL / 50.0 mL

M₁ = 0.104 M

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

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