a) write the net ionic equation for the reaction between HF(aq) and NaO(aq). determine if the value of the equilibrium constant for this reaction b) would the volume of 1.0M NaOH solution needed to completely neutralize 25mL of a .5M HF(aq) be greater than less than or equal to the volume of 1.0M NaOH needed to neutralize 25mL of .5M...
1. An aqueous solution contains 0.28 M hypochlorous acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.)0.14 mol HClO4 0.142 mol NaOH 0.28 mol NaBr 0.29 mol NaClO 0.29 mol HClO4 2. A 1.00 liter solution contains 0.31 M ammonia and 0.40...
14. Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in water? (3 pts) A) nitrous acid B) chlorous acid C) ascorbic acid D) hydrobromic acid E) citric acid 15. Which solution has the highest pH? (3 pts) A) 0.10 M HBr(aq) B) 0.10 M HI (aq) C) 0.10 MHF (aq) D) 0.10 M HCl(aq)...
Determine the pH of each of the following solutions. A. 4.3×10−2 M HI B. 9.95×10−2 M HClO4
Consider the following substances: CH5N, C2H5O2COOH, H3AsO4, KClO2, HC2H2ClO2. For each compound Decide whether the compound behaves as an acid or base in solution Write the equation for the dissociation of the compound in water Write the equilibrium expression for the dissociation in water Calculate the [H+], the [OH-], the pH and the pOH for a solution prepared by diluting...
A 100 mL volume of a 0.100 M weak base (pKb = 5.00) was titrated with 1.00 M HClO4. Find the pH at the following volumes of added acid: 0.00, 1.00, 5.00, 10.00, and 10.10 mL.
16. Exactly 25.00 ml of 0.0685 M HClO4 solution is placed in a flask and titrated with standardized 0.050M NaOH. A. Determine the endpoint of the titration B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution: a.) Initially, 0.00 ml NaOH. b.) 5.00 ml ...
Write the balanced NET ionic equation for the reaction when HClO4 and HI are mixed in aqueous solution. If no reaction occures, write only NR.
Determine the pH 8.8×10−2 M HClO4 and 2.6×10−2 MKOH Express your answer using two decimal places.
How do you find the degree of ionization of the solutions when accounting for the dillution effect of adding 10 mL of water? Also for the second page, how do you calculate pH with a buffer using the Henderson-Hasselbalch equation? Solution 2 - 10.0 mL of 0.1 M HC2H302 +10.0 mL H20 Measured pH_2.42 To determine the [H3O+], account for...