Which two solutions, when mixed together, will undergo a double replacement reaction and form a white, solid substance?
1. NaCl(aq) and LiNO3(aq)
2. KCl(aq) and AgNO3(aq)
3. KCl(aq) and LiCL(aq)
4. NaNO3(aq) and AgNO3(aq)
I know the answers 2 but I have no idea why.. thanks.
A little beyond what we're learning yet it still helped.. thank you !
Could you by any chance give me a list of gasses at STP?
2022 anyone
yep
Elements: Look at the periodic table to see where these are located.
Hydrogen
Nitrogen
oxygen
Fluroine
Chlorine
rare gases (He, Ne, Ar, Kr, Xe, Rn) but these are rarely produced in CHEMICAL reactions.
common compounds:
ammonia, NH3
carbon dioxide, CO2
carbon monoxide, CO
sulfur dioxide, SO2
sulfur trioxide, SO3
nitric oxide, NO
nitrous oxide, N2O
nitrogen dioxide, NO2
nitrogen pentoxide, N2O5
nitrogen trioxide, N2O3
ozone, O3 (technically not a compound)
fuels such as methane, ethane, acetylene, etc.
I see I didn't name by the new rules; i.e., N2O would be dinitrogen monoxide and N2O3 would be dinitrogen trioxide.
For rule c I gave you in the last post, weak acids and weak bases will have an ionization constant (Ka or Kb) and those will be listed in tables. If they are not listed in the Ka or Kb tables they are strong acids or bases. It is easier to list the strong ones. HCl, HBr, HI, H2SO4, HNO3, HClO4, HClO3, are the common strong acids. Common soluble strong bases are KOH, NaOH, (all group IA hydroxides) and Ca(OH)2, Ba(OH)2, Sr(OH)2. MOST others are weak.
Add water to the list of weak electrolytes above. It won't be listed in the Ka or Kb tables but it only weakly ionized.
I hope this gets you one jump ahead.
Come back and see us.
You need to know (and remember) the solubility rules and a couple of other points.
In general, reactions occur for one of three reasons.
a. a gas is formed. Do you know the common gases?
b. a precipitate (and insoluble material) is formed. Do you know the solubility rules?
c. a slightly ionized material is formed. Do you know the weak acids, weak bases, and any other weak electrolytes.
In this question, 2 is the answer because AgCl is formed and that is a white ppt. (rule b in the list of three above). Here is a site that gives the solubility rules.
http://www.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
I can help, also, if you don't know a or c in the list above. Let me know.
Well, let's see if I can shed some light on this! When it comes to double replacement reactions, we need to think about the "switcheroo" that happens between the cations (positive ions) and anions (negative ions). In this case, we're looking for a white, solid substance, which is often an indication of a precipitate forming. So let's go through each option:
1. NaCl(aq) and LiNO3(aq): When we switch the cations, we get NaNO3(aq) and LiCl(aq). Neither of these combinations form a white precipitate.
2. KCl(aq) and AgNO3(aq): Switching the cations gives us KNO3(aq) and AgCl(s). Hey, AgCl is a white solid! We may have a winner!
3. KCl(aq) and LiCl(aq): Switching the cations gives us KCl(aq) and LiCl(aq) again. No white precipitate here.
4. NaNO3(aq) and AgNO3(aq): Switching the cations gives us NaAgNO3(aq) and AgNO3(aq). Again, no white precipitate formed.
So, option 2 (KCl(aq) and AgNO3(aq)) is the correct answer! The double replacement reaction between these two solutions results in the formation of a white solid substance, which is AgCl. Voila!
To determine which two solutions will undergo a double replacement reaction and form a white, solid substance, you need to consider the solubility rules and the potential formation of a precipitate.
In a double replacement reaction, the positive and negative ions of two ionic compounds switch places to form two new compounds. If one of the products of the reaction is insoluble or slightly soluble in water, it will form a solid precipitate. In this case, a white, solid substance is formed.
Here are the solubility rules that will help in determining the solubility of the compounds:
1. Most nitrates (NO3-) are soluble.
2. Most chlorides (Cl-) are soluble, except for chlorides of silver (Ag+) and lead (Pb2+).
3. Most compounds containing alkali metal ions (Group 1 elements, such as Na+ and K+) are soluble.
4. Most compounds containing ammonium ions (NH4+) are soluble.
Now, let's analyze the given options:
1. NaCl(aq) and LiNO3(aq): Both compounds contain alkali metal ions and nitrate ions, which are soluble according to the solubility rules. So, they are not likely to form a precipitate.
2. KCl(aq) and AgNO3(aq): KCl is soluble, as it contains an alkali metal ion (K+). AgNO3 contains the silver ion (Ag+), which is insoluble according to the solubility rules. Hence, a precipitate of silver chloride (AgCl) will form, which is a white, solid substance.
3. KCl(aq) and LiCL(aq): Both compounds contain alkali metal ions (K+ and Li+), which are soluble according to the solubility rules. So, they are unlikely to form a precipitate.
4. NaNO3(aq) and AgNO3(aq): Both compounds contain soluble ions, sodium (Na+), and nitrate (NO3-), without any insoluble ions.
Based on the solubility rules, the only option that will form a white, solid precipitate is option 2: KCl(aq) and AgNO3(aq).