Since KHP is an unknown (name for a) chemical compound the molarity can not be calculated by lack of data.
The molar mass (m) of KHP ANDthe number (n) of H+ per mol KHP (maybe 1 when monoprotic?) is necessary for calculation, according to this formula:
(M*V)NaOH = (n*mass/m)KHP
so:
[OH-] (mol.L-1) * 0.02850 (L NaOH sol'n) = n (mol H+.mol-1 KHP) * 0.7154 (g KHP) / m (g.mol-1 KHP)
1.3g
Molarity = moles of solute(CuSO4)/volume of solution(Liters) 0.967 grams CuSO4 (1 mole CuSO4/159.62 grams) = 0.00606 moles CuSO4 Molarity = 0.00606 moles/0.020 liters = 0.303 Molarity
The molarity is 6.
Looks as if you will need to calculate the pH of the final solution. The formula you need will be [H+] = 1 x 10-6 M.
You can prove there is glucose in a sample by using Benedict's Solution. Heat up the sample, and add the Benedict's Solution. Assuming the solution is clear, if glucose is present it will change colour to red, or yellow, or green. If not, it will stay clear.
What is the molarity of an HCl solution if 43.6 mL of a 0.125 M KOH solution are needed to titrate a 25.0 mL sample of the acid according to the equation below?
The HCL concentration is 1.2M or 1.2N
22
1.3g
.430
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M
1.0 Moles
Molarity = moles of solute(CuSO4)/volume of solution(Liters) 0.967 grams CuSO4 (1 mole CuSO4/159.62 grams) = 0.00606 moles CuSO4 Molarity = 0.00606 moles/0.020 liters = 0.303 Molarity
1.00x10^-7
10.332
There are answers elsewhere on the web. In summary, a titrand is the solution (or other substance) which one has in a conical flask or beaker into which the titrant is titrated from a burette.
The molarity is 6.