A 75.0 mL aliquot of a 1.60 M solution is diluted to a total volume of 258 mL. A 129 mL portion of that solution is diluted by adding 125 mL of water. What is the final concentration? Assume the volumes are additive.

Thus the final concentration is 0.236 M

Explanation:

According to moalrity equation:

= Molarity of stock solution = 1.60 M

= volume of stock solution = 75.0 ml

= molaity of diluted solution = ?

= volume of diluted solution = 258 ml

For second dilution:

= Molarity of stock solution = 0.465 M

= volume of stock solution = 129 ml

= molaity of diluted solution = ?

= volume of diluted solution = (129+125) = 254 ml

Thus the final concentration is 0.236 M

b. acid is the correct answer @jayxboof all social media

acid : acids are those which accepts an electron-pairs.

base : bases are those which donates ab electron-pairs.

alkali : it is a base that dissolves in water. it is basically a base and the ph greater than 7.

hydroxide ion : it is a poly-atomic ion which is negatively charged.

i think is conclusions.i think so