200" cm"^(2) of an aqueous solution of a protein contains 1.26 g of the protein. The oxmotic pressure of such a solution at 300 K is found to be 2.57xx10^(-3) bar. Calculate the molar mass of the protein.
300 mL of an aqueous solution of a protein contains 2.52 g of the protein. If osmotic pressure of such a solution at 300 K is 5.04xx10^(-3) bar, the molar mass of the protein in g mol^(-1) is
If the osmotic pressure of glucose solution is 1.52 bar at 300 K. What would be its concentration if R = 0.083L bar "mol"^(-1)"K"^(-1) ?
A decimolar solution of K_4[Fe(CN)_6] at 300K is 50% dissociated, then, osmotic pressure of the solution is
At 300 K, a one litre solution of sucrose (molecular weight : 342 ) was prepared by dissolving 40 g of sucrose. What is the approximate osmotic pressure (in kPa) of solution at the same temperature ? (R = 8.314 xx 10^6 cm^3 Pa K^(-1) mol^(-1))
H_3A is a weak triprotic acid (K_(a_1) =10^(-5) ,K_(a_2) =10^(-13) ) . What is the value of pX of 0.1 M H_3 A(aq.) solution ? Where pX =- log X and X = ([A^(3-)])/([HA^(2-)])
At 10^@C , the osmotic pressure of urea solution was formed to be 500 mm. The solution is diluted 'x' times and the temperature raised to 25^@C when the osmotic prssure was noticed to be 105.3mm, then 'x' is
NARENDRA AWASTHI-DILUTE SOLUTION-Level 3 - Match The Column
