Potassium Hydrogen Phthalate
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)KHPso:[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)
molar mass of KHP is 204.2g/mole. the formula for KHP is C8H5O4K therefore, (12.01*8)+(1.008*5)+(16*4)+39.1 = 204.2g/mol
KHP
122.5g
The term molar it refers a form to know the concentration of a solution, and it is equivalent to a molar unit in a litre of solvent 1 Molar (1M) = 1 mole (molecular weight from the structure you are interested in) / 1000 mL or 1 L. Milimolar is the thousandth part from a solution 1M
KHC8H4O4(aq) + NaOH(aq) --> KNaC8H4O4(aq) + H2O(l). The molar mass of KHP is approximately 204.22 g/mol. 1.54g of KHP is equivalent to 0.00754 mol of KHP. 1 mole of NaOH reacts per mole of KHP, so .00754 mol of NaOH are needed.
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)KHPso:[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)
molar mass of KHP is 204.2g/mole. the formula for KHP is C8H5O4K therefore, (12.01*8)+(1.008*5)+(16*4)+39.1 = 204.2g/mol
no
71.0800g/mole
KHC8H4O4(aq) + NaOH(aq) → KNaC8H4O4(aq) + H2O(l) NaOH(aq) + KHP(aq) => Na+ + KP- + H2O(l)
KHP
Perchloric acid is a strong acid, whereas potassium hydrogen phthalate (KHP) is a weak acid. Therefore, perchloric acid will protonate KHP to form phthalic acid. In other words, even though both are considered acids, KHP is more basic than perchloric acid (when you compare their pKa or Ka, the true measure of acid strength). I'm not entirely sure what you mean by "standardized" however. Do you mean doing a titration? Often a solution of KHP is used to calibrate a pH meter because it's pH in solution is very stable. I would be surprised if a titration was done with perchloric acid and KHP however, but I'm not sure what else you could mean by asking why an acid is standardized using KHP. KHP is the primary standard used for the standarization of perchloric acid, usually 0.1M HCLO4 in concentration. It is the recommended primary standard in the pharmaceutical industry for analytical testing using perchloric acid for non-aqueous titration determinations. The protonation of KHP to phthalic acid when reacted with perchloric acid can be determined stoichiometrically. Using a dried KHP standard of known purity allows the determination of HCLO4.
The same number of moles for each.
KHP (potassium hydrogen phthalate) is available extremely pure (which is always good for a primary standard) and gives a very sharp end-point especially with Crystal Violet Indicator
vzcvz
the volume would not be accurate, making the molarity inaccurate.