Help m A 280.0 sample of neon gas exerts a pressure of 660.0 mm Hg at 26.0°C. Assuming that the pressure remains constant, at what temperature in would the volume change to 440.0 ml?

469.9K

Explanation:

Using Charles's law equation:

V1/T1 = V2/T2

Where;

V1 = initial volume (ml)

V2 = final volume (ml)

T1 = initial temperature (K)

T2 = final temperature (K)

Based on the information provided:

V1 = 280.0ml

V2 = 440.0 ml

T1 = 26.0°C = 26 + 273 = 299K

T2 = ?

Using V1/T1 = V2/T2

280/299 = 440/T2

0.936 = 440/T2

T2 = 440 ÷ 0.936

T2 = 469.9K

the ratio of the conjugate base to the acid required to attain the desired ph.