One drop 6 M NaOH is added to 0.5 mL of 0.04 M CuSO4 solution. What is the identity of the substance that causes cloudiness in this reaction?
Enter the chemical formula.
One drop 6 M NaOH is added to 0.5 mL of 0.04 M CuSO4 solution. What...
One drop 0.2 M Na2C2O4 is added to 0.5 mL of 0.04 M CuSO4 solution. What is the identity of the substance that causes cloudiness in this reaction? Enter the chemical formula.
One drop of 2.5 M KSCN solution is added to 0.5 mL of 0.10 M Fe(NO3)3. After the solution is mixed, 1.0 mL of 0.125 M EDTA solution is added. Enter the chemical formula of the major iron complex in solution after the addition of EDTA
As 50.0 mL of 0.10 M NaOH is added to 100.0 mL of 0.5 M NaOH, what happens to the pH of the original solution? does it increase or decrease
0.5 mL of a 0.04 M CoCl2 solution is combined with 1.5 mL deionized water. What is the molarity of the solution?
1) 0.5 ml of 1 M NaOH was added to 0.5L of a 100mM buffer solution at pH=7.0. Calculate how the pH value is affected by this addition if a pKa value of the buffer is 7.47. b) 1ml of 0.01mM HCl is added to 10L of pure water. What is a pH of this solution?
6. 48.6 mL of a 0.100 M NaOH solution is needed to react with 20.0 mL of an unknown concentration of HCl solution. What is the concentration of the HCl solution? 7. A colorless liquid has a composition of 84.1% carbon and 15.9% hydrogen by mass. Determine the empirical formula. Also, assuming the molar mass of this compound is 114.2 g/mol, determine the molecular formula of this compound. 8. What is the concentration of HCl in the final solution when...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2? 6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
a.)100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint. 1.) 150 mL of 1 M NaOH 2.) 200 mL of 1 M NaOH 3.) 50 mL of 1 M NaOH 4.) 100 mL of 1 M NaOH 5.) 5.00 mL...
0.85 mL of 2.4 M NaOH was added to neutralize 45.0 mL of a H3PO4 solution. a) write the balanced molecular equation b) calculate the concentration of the phosphoric acid solution 6. 0.85 mL of 2.4 M NaOH was added to neutralize 45.0 mL of a H3PO4 solution. (10 points) a) Write the balanced molecular equation. b) Calculate the concentration of the phosphoric acid solution.
A 14.2 ml solution of 0.036 M CaCl2 is mixed with 10.1 ml of 0.04 M BaCl2. Aqueous KF is added. Calculate the fluoride ion concentration (in M) that will separate the metal ions. Enter a number to 4 decimal places.Ksp for CaF2 = 3.2x10−11 Ksp for BaF2 = 1.5x10−6