(a) Na2CO3 is an ionic salt which completely dissociates into Na+ and CO32- according to equation :
Na2CO3 (aq) 2 Na+ (aq) + CO32- (aq)
Given : concentration of Na2CO3 = [Na2CO3] = 0.015 M
[Na+] = 2 * [Na2CO3]
[Na+] = 2 * (0.015 M)
[Na+] = 0.030 M
[CO32-] = [Na2CO3]
[CO32-] = 0.015 M
(b) Fe(NO3)3 is an ionic salt which completely dissociates into Fe3+ and NO3- according to equation
Fe(NO3)3 (aq) Fe3+ (aq) + 3 NO3- (aq)
Given : concentration of Fe(NO3)3 = [Fe(NO3)3] = 0.75 M
[Fe3+] = [Fe(NO3)3]
[Fe3+] = 0.75 M
[NO3-] = 3 * [Fe(NO3)3]
[NO3-] = 3 * (0.75 M)
[NO3-] = 2.25 M
3. Determine the concentration of each ion in solution. (a) [Na2CO3]=0.015 M (b) [Fe(NO3)3] = 0.75...
What is the concentration of Cu2+ (aq) in a solution that was originally 0.015 M Cu(NO3)2 and 0.1M NH? The Cu2+ ion forms the complexion Cu (NH3)42-K-4,9x10 12 Show your calculations.
What is the concentration of the Cu²⁺(aq) ion in a 0.015 M Cu(NO₃)₂ solution that is also 1.0 M NH₃? The Kf for Cu(NH₃)₄²⁺ = 4.8 x 10¹² .
You will be preparing a standard solution by mixing 2 solutions: 0.200 M Fe(NO3)3 and 0.00200 M KSCN. The concentration of the M Fe(NO3)3 solution is 100 times greater than the concentration of KSCN solution. What is the purpose of using a large concentration of Fe(NO3)3 and a small concentration of KSCN to make the standard solution? EXPLAIN
a. A 10 ml calibration solution is made by mixing 5 mL of 0.200 M Fe(NO3)3, 1.50 mL of 2.00X10-3 M KNCS, 1 mL of 0.100 M nitric acid and 2.50 mL H20. What is the final concentration of only the NCS-ion? b. If 1.00 ml of this solution is then diluted to a final volume of 25.00 ml with DI water. What is the new concentration of NCS?
The actual concentration of the stock [Fe(NO3)3] solution you will use in lab will be posted on D2L. Be sure to record the concentration value matching YOUR lab room and use it in your laboratory worksheet! Consider test tube #5 that you will prepare in Part 1 of the laboratory (Table A). If your dilute solution of Fe(NO3)3 had a concentration of 0.00087 M, predict the initial concentration of the Fe3+ ions, [Fe3+]0 in test tube #5, once you have added...
11. Which of the following is expected to be insoluble in water? A. Na2CO3 B. Fe(NO3)3 C. KS04 D. AGNO3 E. ZnS 12. Which of the following has the lowest oxidation number? A. S in H2SO4 B. Cr in KiCrO4 C. Xe in XeFG D. Clin Ca(CIO3)2 E. Mn in KMnO4 13. Which of the following correctly defines "molarity"? A. mol solute/L solution B, mol solute/mL solvent C. mol solute/kg solvent D. mol solute/L solvent E. ky solute/mol solution 14....
If 2.63 g Fe(NO3), is dissolved in enough water to make exactly 460 mL of solution, what is the molar concentration of nitrate ion? M of Fe(NO3)3=241.86 g/mole
Determine the concentration of nitrate ions after 126.0 mL of 0.121 M solution of Cu(NO3)2 and 193.0 mL of 0.215 M solution of Fe(NO3)3 are mixed together. Assume that volumes are additive.
Determine the concentration of nitrate ions after 126.0 mL of 0.121 M solution of Cu(NO3)2 and 193.0 mL of 0.215 M solution of Fe(NO3)3 are mixed together. Assume that volumes are additive. A). 0.887 M B). 0.486 M C). 0.336 M D). 0.168 M E). 0.178 M
The metathesis reaction between iron (III) nitrate and sodium sulfide is shown below 2 Fe(NO3)3(aq) + 3 Na2S (aq) ➝ 6 NaNO3(aq) + Fe2S3(s) How many grams of solid iron (III) sulfide can be produced by the reaction of 250.0 ml of 0.400 M iron (III) nitrate solution with 350.0 ml of 0.250 M sodium sulfide solution? Determine the final concentration of each ion in solution at the end of the precipitation reaction. Na+ NO3– Fe+3 S–2