4. A sample of gas occupies a volume of 80.OmL at a pressure of 0.50 atm and a temperature of
0.0°C. What will its volume be at a pressure of 1.50 atm and a temperature of 50.0°C?

The volume will be 31, 55 ml

Explanation:

We use the gas formula, which results from the combination of the Boyle, Charles and Gay-Lussac laws. According to which at a constant mass, temperature, pressure and volume vary, keeping constant PV / T. We convert the unit Celsius into Kelvin:

0 ° C = 273K, 50 ° C = 273 + 50 = 323K

(P1x V1)/T1= (P2xV2)/T2

(0,5atm x 80ml)/273K =(1,5 atmxV2)/323K

0,147 atmx ml/K= (1,5 atmxV2)/323K

V2= (0,147 atmx ml/Kx 323K)/1,5atm= 31,55 ml

b is the correct

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.