(Answer the questions and turn in this at the beginning of the first week of Ani
ID: 706619 • Letter: #
Question
(Answer the questions and turn in this at the beginning of the first week of Anion Lab) 1. Based on the solubility table given in Table 1, which cation (or cations) will form soluble salts with all Sx anions (So, Co, Po, Cr,r, NO,)? Can this cation be used to identify potential presence of any of these six anions in an unknown solution? Explain your answer. (3pts) 2. What cation reagent you will first use to test the known anion solutions? What do you need to observe carefully? (2pts) 3. List the reagents you will use in order to learn more about differences in chemistry of silver chloride and silver iodide. (2pts) 4. To confirm the presence of nitrate ion, you will be performing a so-called brown ring test. Describe briefly how you will do the test (show at least three steps) (3pts)Explanation / Answer
Question 1
Any salt of first group metal (Li+, Na+, K+, Rb+, Cs+) are readily soluble in water.
In connection with the given question, the cations Na+ and K+ will form readily soluble salts with all six anions (SO42-, CO32-, PO43-, Cl-, I-, NO3-).
Reason: The solubilities are greater than 11.1 - 179 g, which is good enough to decide the solubility of the corresponding salts.
No, the cations Na+, K+ can't be used for the identification of the potential presence of any of the given six anions in an unknown solution using K+.
Explanation: the cations Na+ and K+ form soluble compounds with the given six anions. There is no formation of the deductible amount of precipitate.
For example, Ca2+ reacts with PO43- ion to give the appreciable amount of Ca3(PO4)2 as a precipitate. Therefore, we can identify the phosphate ion using Ca2+ by the naked eye.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.