A75.0 ml 75.0 ml aliquot of a 1.70 m 1.70 m solution is diluted to a total volume of 278 ml. 278 ml. a 139 ml 139 ml portion of that solution is diluted by adding 165 ml 165 ml of water. what is the final concentration? assume the volumes are additive.

0.210 M

Explanation:

A 75.0 mL aliquot of a 1.70 M solution is diluted to a total volume of 278 mL.

In order to find out the resulting concentration (C₂) we will use the dilution rule.

C₁ × V₁ = C₂ × V₂

1.70 M × 75.0 mL = C₂ × 278 mL

C₂ = 0.459 M

A 139 mL portion of that solution is diluted by adding 165 mL of water. What is the final concentration? Assume the volumes are additive.

Since the volumes are additive, the final volume V₂ is 139 mL + 165 mL = 304 mL. Next, we can use the dilution rule.

C₁ × V₁ = C₂ × V₂

0.459 M × 139 mL = C₂ × 304 mL

C₂ = 0.210 M

answer: find it ur self

explanation:

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2