What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with Ka = 3.5x10-8? The equation for the dissociation of hypochlorous acid is: %3D HOCI(aq) + H2O(1) H30*(aq) + OCI (aq) Answer:
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- For the reaction Na + H2O --> NaOH + H2, which is the value of delta S - balance first -In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid ( 1mL ≎0.0031g Na2O) What is the normality of NaOH?Calculate the pH of a 2.00 M Na2CO3 given that the pKa’s of the first and second dissociation of H2CO3 (aq) acid are 6.37 and 10.32, respectively.
- When acidulated water (dil.H2SO2solution) is electrolysed, will the pH of the solution be affected? Justify your answer.In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid (1mL = 0.0031g Na20) What is the normality of NaOH? Additional instructions: Make it handwritten Include up to 4 decimal places Please include explanations of the process Thank you so much!The freezing point of a 0.100 M acetic acid (CH3COOH) solution is determined to be-0.1878 C. Estimate the percent dissociation of acetic acid in this solution. Is it a strong orweak electrolyte? Note that acetic acid produces acetate (CH3COO-) and hydrogen (H+) ionswhen it is dissolved in water.
- .Consider an aqueous solution of pyridine, C5NH5(aq), with F = 5.0 mM, at 1 bar and at 298 K. Pyridine is a weak Brønsted-Lowry base. Write down the equation for charge balance.Soil water with 10^-3 N alkalinity is in equilibrium with a soil gas in which PCO2= 10^-1 atm. If the soil water is pumped from the ground and exposed to air, what will the equilibrium pH be?Consider an aqueous solution of pyridine, C5NH5(aq), with F = 5.0 mM, at 1 bar and at 298 K. Pyridine is a weak Brønsted-Lowry base. Structure of pyridine, Write all the relevant chemical reactions among the species
- Give the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10If the equilibrium constant for a reaction A + B <=> 2C is measured as Keq = 1.318. What would the value be for the same reaction if written as 2C <=> A + B. Keq' = ____. 3 sig. fig.Calculate the pH if 0.30 M solution of acetic acid at 25 degree Celsius. Ka for acetic acid = 1.8 x 10^-5