Answer:
Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions.
Explanation:
The student have in solution Ag⁺ and Cu²⁺ ions but he just want to analyze the silver, that means he need to separate ions.
Centrifuging the solution to isolate the heavier ions <em>FALSE </em>Centrifugation allows the separation of a suspension but Ag⁺ and Cu²⁺ are both soluble in water.
Adding enough base solution to bring the pH up to 7.0 <em>FALSE </em>At pH = 7,0 these ions are soluble in water and its separation will not be possible.
Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions <em>TRUE </em>For example, the addition of Cl⁻ will precipitate the Ag⁺ as AgCl(s) allowing its separation.
Evaporating the solution to recover the dissolved nitrates. <em>FALSE</em> . Thus, you will obtain the nitrates of these ions but will be mixed doing impossible its separation.
I hope it helps!
Answer: 0.943 g/ml
Explanation:
Mass of added solution: (26.153g - 23.022g) = 3.131g
Volume of solution = 3.32 ml
Density = Mass/Vol
Density = (3.131g)/3.32 ml) = 0.9431 g/ml
0.943 g/ml for 3 sig figs
<span>Topic & Statement (ask a question)
Conduct Research
Form a Hypothesis
Conduct an Experiment
Collect Data
Analyze Results
Form Conclusions
Report & Present</span>
Answer:
The ionic compounds are chemical compounds composed of ions, which is held together by electrostatic forces termed ionic bonding.
True- the number of protons in an atom is also the atomic mass!!
