Suppose 1.30 g of NaNO2 is added to enough 0.20 M HNO2 to make exactly 50 mL of solution. What is the expected pH of the resulting solution? How do I know what the Ka for this problem is? Do I need to look it up in my textbook?
Suppose 1.30 g of NaNO2 is added to enough 0.20 M HNO2 to make exactly 50...
A buffer solution consists of 0.10 M HNO2 and 0.20 M NaNO2. If 0.010 moles of sodium hydroxide are added to 200. ml the solution , what is the new pH of the solution (pKa (HNO2) = 3.40)?
A 1.00 L solution contains 20.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.56? Ka (HNO2) = 4.0 × 10–4.
1) 20. mL sample of 0.20 M HOCl is added to 25.0mL of 0.20M KOH. What is the pH of the solution? -8 HOCl (Ka = 3.5 x 10 ) 2) The ideal pH for the pool is 7.4. What is the ratio of (OCl- ) to (HOCl) needed to maintain the swimming pool at a pH of 7.4? 3) What would be the new pH if you added 0.3 moles of NaOH to 1.0L of the pool water at...
with work please 4) Suppose 50 mL of 0.1 M NaOH is added to 50 mL of 0.1 M HC2H302 (Ka = 1.8 X 10-5). This is a titration at its equivalence point. Calculate the pH of the resulting mixture.
A solution is prepared by dissolving 0.5892 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution? I do not know if the answer of 0.00187 or 1.87 x 10^ -3 is correct. It is incorrect in my perspective, so i do not expect that answer, if you think...
1) enough of solution A (0.16 M HAc) is added to solution B (6.4x10^-3 M NaAc) to form a solution that is equimolar in HAc and Ac-. What volume of solution A must be added to 50mL of solution B to produce an equimolar solution? 2) You are asked to prepare 10.00 mL of buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A-). The target pH of the buffer solution is 5.25. Ka of...
If 1.85 g MgO is combined with enough 1.00 M HCl to make 100.0 mL of solution in a coffee-cup calorimeter, the temperature of the resulting solution increases from 21.3°C to 35.7 °C. Calculate the enthalpy change for the reaction per mole of Mgo. Assume that the specific heat capacity of the solution is 4.18 J/g.K, and the density of the solution is 1.00 g/mL. A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base...
I need help with questions 1,3,4,5 1.0.15 M ammonium chloride is added to a 0.05 M solution of ammonia. How does the pH change? NHs(aq) + H2O(1) NH(aq) + OH(aq) A. pH goes up B. pH goes down C. pH does not change 2. Which of the following would make buffer system? A. a weak asid and NaCl B. a weak acident's conjugate base C. a strong acid and a weak acid D. alveak acid and a strong acid E....
Question 16 of 24 Determine the pH of a buffer that is 0.55 M HNO2 and 0.75 M KNO2. The value of Ka for HNO, is 6.8 x 10-4 1 2 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. HNO3(aq) + H2O(1) H,O*(aq) + NO, (aq) Initial (M) Change (M) Equilibrium (M) RESET 2x 0 0.55 0.75 6.8.10 0.55. 2x 0.56 - 2x 0.75 + x 0.75 - X 0.55 -...
Hello I need help with number # 2. as it’s asking me to make predictions and fill in the first column of Part A of this experiment Please help as I don’t know what problem two means by predicting for the first column? d. 2.5 xIO 10.t 2. Make predictions and fill in the first column of Part A of this experiment 3. What is the app roximate expected pH ofa 0.030 M HNo, solution? hat is the final pH...