how do you calculate pH of super concentrated acid (such as 98% sulphuric acid or 99,5% ethanol)?
Ans: The pH can be calculated for the sulfuric acid only, as the ethanol is neutral organic alcohol and pH is not applicable to it.
Now, to calculate the pH of the super concentrated sulfuric acid, first we should know the moles of sulfuric acid present in one litre volume. For that we should first calculate the Mass (M) of sulfuric acid in 1 L volume based upon the % purity and its density.
Density of the super concentrated H2SO4 = 1.84 g/cm3 (from Litt.)
Purity of the super concentrated acid = 98 %
Molecular weight (molar mass) of the sulfuric acid = 98.1 g/mol
Mass of acid in 1L volume = 1.84 * 1000 * 0.98 = 1803.2 g
Number of moles in the above sulfuric acid weight
= weight of sulfuric acid / molar mass of the acid = 1803.2 / 98.1 = 18.38 Moles
Hence, the concentration of [H+] = 18.38 x 2 = 36.76 mol/L (sulfuric acid molecule has two protons)
pH = -log [H+]
pH = -log [36.76]
pH = 1.57
how do you calculate pH of super concentrated acid (such as 98% sulphuric acid or 99,5%...
1. how can a 98% sulphuric acid be diluted to get a concentration of 0.05 mol per L?
How do you calculate the pH of a solution containing a weak acid or a weak base? Please write down the general formula for finding the H3O+ ion concentrations in case of a weak acid Please explain the common-ion effect in terms of Le Châtelier. You might want to use the general chemical equation for an acid ionization HA + H2O ↔ A- + H3O+ to help you explain the phenomenon. How do you calculate the degree of ionization? Please...
How do pH, propionic acid, and propionate change when HCl, a strong acid solution, with a final concentration of 0.0005 mole/L, is added to the solution containing 10-3 M sodium propionate? HCl is added from a concentrated stock solution, so the volume change is negligible.
How do you find the Molarity and calculated pH? A. pH of Acid Solutions: Compare and explain the observed values of pH for these two acids.
calculate the pH of the conjugate base of a weak acid NaAcid ? What equations do you use to calculate the p e to calculate the pH of a defined mixture of HAcid and NaAcid? What equations do you use to calculate the pH calculate the final pH of a defined buffer after adding Strong Acid or Strong Base?
Commercially available concentrated phosphoric acid is 15.2M . Calculate the volume of concentrated phosphoric acid required to prepare 1.50 L of 1.50M solution. Volume = L
TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
A test procedure requires 500mL of a 4N phosphoric acid solution. The concentrated phosphoric acid available has a specific gravity of 1.69 and an assay of 85%. How would you prepare this solution? (MW H3PO4 = 98) (Valence is 3)
How do I calculate the theoretical yield and percent yield of the reaction below? I used 0.120 g of 4-aminobenzoic acid, 2.0 mL of ethanol, and 0.5 mL of concentrated sulfuric acid The mass of the final product was 0.42 g to O CH2CH2OH o H2N- HN OH H2SO4 OCH CH3 4-Aminobenzoic acid Benzocaine
If concentrated phosphoric acid is 14.7 M, how many ml of acid would you use to make 400 ml of 2N phosphoric acid?