Explain why the anionic solution need to be acidified during identification of anions
Test for halide : Add AgNO3. Gives precipitate of silver halide if halide anion present.
To test for halide (Cl-, Br-, I-) ions, the sample is acidified (with dilute HNO3) before adding AgNO3 for testing. This is because , if carbonate ion is present (CO3 2-) , then it will form a precipitate of silver carbonate ( Ag2CO3) with AgNO3 , and so, a positive test will be obtained even if halide anions are not present. But, if acid is added, then the acid H+ reacts and removes the carbonate ions :
2H+ + CO3 2- = CO2 + H2O .
CO2 is evolved as a gas, and carbonates are removed from solution.
Test for sulfate : Add BaCl2. Gives white precipitate ( of BaSO4) if sulfate anion present.
When testing for sulfates:
If sulfites are present in solution, BaSO3 precipitate will form after adding BaCl2 , and so, a positive test is shown even if no sulfate anion is present. But this BaSO3 is soluble in acids. So, if the sample is acidified, then BaSO3 won't precipitate.. (the acid can also be added after adding BaCl2 to distinguish sulfite and sulfate)
Explain why the anionic solution need to be acidified during identification of anions
identification and selected ions
INSTRUCTOR REPORT FOR EXPERIMENT 14 Identification of Selected Anions Naci | Nal NaBr Na so, Naso, Na.co. Unknown Unknown Na PO, INo. A AgNO, Test Addition of AgNO, solution Addition of dil. HNO, 127 - B. BaCl, Test Addition of BaCl, solution Addition of dil. HCI c. Organic Solvent Test Color of decane layer D. Formula of anion present in the solution tested.
PLEASE EXPLAIN! I NEED HELP. IT WOULD MEAN A LOT.
Order the anionic compounds from the most basic to least basic? 3) 1) 2) Magnify Select One Strongest base Second strongest Match With B 3) Weakest base C 2)
Testing for Cations and Anions - Lab 6 B. Tests for Negative lons (Anions) Procedure Observations Observations for unknown BI Chloride test ar B.2 Sulfate test SO? B.3 Phosphate test PO 3.4 Carbonate test 00 Identification of the negative ion in the unknown solution From your test results, what negative ion (anion) is present in your unknown? Explain your choice. C. Writing the Formula of Your Unknown Salt Unknown sample number C. Cation Name Name Anion C.2 Formula of the...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6 H...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H202 + 2 MnO - +61 +502...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO4 - +6H→ 5...
3. A 25.00 mL of Commercial Peroxide solution is titrated with 0.200 M acidified KMnO4 solution according to the balanced equation provided below. The initial volume reading from the buret is 4.15 mL. The final volume of the buret reading is 15.23 mL. A. Why using an indicator for this redox titration experiment is unnecessary? How will determine the end point of the titration? B. Determine the molarity of the H2O2 solution? 5 H2O2 + 2 MnO. - + 6...
Explain the concepts of acculturation and intensity of ethnic identification and why understanding them is important to marketers.
1. Explain why a buffer solution should be used to prepare for the fluorescein solution. -2. Indicate the wavelength of a shoulder in an absorption band. Explain why a shoulder exists in the absorption band. 23. Calculate the mole ratio of dianion to monoanion of fluorescein at pH 7.4 (use the Handerson-Hasselbalch equation to calculate the ratio). Calculate the absorbance ratio of the dianion to monoanion from the absorption spectrum. Can you claim that since the absorbance is proportional to...