Fe 3+ + SCN- --> FeSCN 2+
<span>.......Fe 3+.......SCN-.........FeSCN 2+ </span>
<span>I.......0.04..........0.001.............. </span>
<span>C........-x...............-x............. </span>
<span>E.....0.04-x.....0.001-x...........x </span>
<span>Keq = 203.4 = x / (0.04-x)(0.001-x) </span>
<span>203.4 = x / (x^2 - 0.041x + 4x10^-5) </span>
<span>203.4x^2 - 8.34x + 0.00094 = x </span>
<span>203.4x^2 - 9.34x + 0.00094 = 0 </span>
<span>x = -0.0001M or 0.0458M </span>
<span>therefore, according to the calculated Keq, all of the SCN- and Fe 3+ would be fully converted into FeSCN 2+</span>
Convert HCl and H2O to moles.
36.0 g of HCl = 0.987 moles HCl
98.0 g of H2O = 5.44 moles H2O
Based on the stoichiometric ratio for HCl,
there are 0.987 moles of H and 0.987 moles of Cl.
For H₂O, according to the stoichiometric ratio, you have 10.88 moles of H and 5.44 moles of O.
Combining them:
11.867 moles H
0.987 moles Cl
5.44 moles O
Revert the moles back to grams, then divide by the total mass and multiply by 100 for the percentage by mass.
11.867 moles H = 11.96 g H
0.987 moles Cl = 34.99 g Cl
5.44 moles O = 87.03 g O
11.96/(36.0+98.0)(100) = 8.93% for H
34.99/(36.0+98.0)(100) = 26.11% for Cl
87.03/(36.0+98.0)(100) = 64.96% for O.
Answer:
The categorization of strong, weak, and non-electrolytes is detailed below, based on the examples presented in the question.
Explanation:
A strong electrolyte fully dissociates or nearly so in an aqueous environment; typically, strong acids, bases, and salts fall under this category. Examples of strong electrolytes include:
- Hydrochloric acid, HCl
- Calcium hydroxide, Ca(OH)2
- Potassium chloride, KCl
A weak electrolytepartially ionizes in solution; weak acids and bases are primary instances. Examples consist of:
- Methylamine, CH3NH2
- Hydrofluoric acid, HF
A non-electrolytedoes not dissociate in an aqueous medium. Examples of non-electrolytes are:
- Sucrose, C12H22O11
- Methanol, CH3OH
