Asolution of 62.4 g of insulin in enough water to make 1.000 l of solution has an osmotic pressure of 0.305 atm at 25°c. based on these data, what is the molar mass of insulin?

Molecular Mass of insulin = 5004

Explanation:

Mass of insulin = 62.4 g

Volume of the solution = 1.00 L

Osmotic pressure = 0.305 L

Temperature = 25 °C = 25 + 273 = 298 K

PV = nRT

Where,

P = osmotic pressure

V = Volume of the solution

n = No. of moles

R gas constant = 0.08206  L atm K^{-1} Mol^{-1}

T = Temperature

PV = nRT

n = 0.01247

No. of mol = Mass in g/molecular mass

Molecular mass = Mass in g/No. of mol

Molecular mass = 62.4/0.01247

                          = 5004

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.

the electrical  conductivity  of asolution  of an electrolyte is measured by determining the resistance of thesolution  between two flat or cylindrical electrodes separated by a fixed distance.