Which of the following salts is slightly soluble in water?
A. AgCl
B. CaSO4
C. Na2CO3
D. PbCl2?
You question is very ambiguous. AgCl is the least soluble, Na2CO3 is the most soluble, CaSO4 & PbCl2 solubilities are in the same order of magnitude.
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The salt calcium sulfate is sparingly soluble in water with a solubility of 0.209 g/100 mL of water at 30 degree C. If you stirred 0.550 g CaSO4, into 1.000 mL water at 30 degree C, what would the molarity of the resulting solution be? How many grams of CaSO4 would remain undissolved? The balanced equation for the oxidation of ethanol to acetic acid by potassium dichromate in an acidic aqueous solution is 3C2H5OH(aq) + 2 K2Cr2O7(aq) + 16HCl(aq) xrarr 3 CH3COOH(aq) + 4 CrCl,(aq) + 4 KCl(aq) + 11H2O(l) What volume of a 0.600 M potassium dichromate solution is needed to generate 0.166 mol acetic acid (CH3COOH) from a solution containing excess ethanol and HCl?
From: www.chegg.com
Well, it seems we've got ourselves a solubility showdown! Let's see which salt comes out on top.
A. AgCl: Not a fan of water. AgCl is insoluble, so it's out of the running. Sorry, silver chloride!
B. CaSO4: This one isn't very soluble either. Calcium sulfate is like that distant cousin at a family gathering who never wants to join the conversation. So, it's a no-go for calcium sulfate.
C. Na2CO3: Bingo! Sodium carbonate has a bit of a love affair with water. It's slightly soluble, making it the winner in this salty competition.
D. PbCl2: Unfortunately, lead chloride is a wallflower when it comes to dissolving in water. It prefers to keep to itself and remain insoluble.
So, the answer is C. Na2CO3. Congrats, sodium carbonate! You managed to out-solubilize the competition. Keep making those water molecules blush!
To determine which of the following salts is slightly soluble in water, we need to understand the concept of solubility. Solubility refers to the ability of a substance to dissolve in a solvent, such as water. A salt is considered slightly soluble if it only partially dissolves in water and forms a relatively small amount of dissolved ions.
One way to determine the solubility of salts is by referring to solubility rules, which provide guidelines for predicting whether a salt is soluble or insoluble in water. Here are the solubility rules for the salts in question:
1. Most chloride (Cl-) salts are soluble, except for those of silver (Ag+) and lead (Pb2+).
2. Most sulfate (SO42-) salts are soluble, except for those of calcium (Ca2+), strontium (Sr2+), and barium (Ba2+).
3. Most carbonate (CO32-) salts are insoluble, except for those of sodium (Na+) and potassium (K+).
Now let's apply these rules to the given options:
A. AgCl: According to the solubility rules, silver chloride (AgCl) is insoluble in water. Therefore, it is not slightly soluble.
B. CaSO4: Calcium sulfate (CaSO4) is listed as insoluble in the solubility rules. Thus, it is not slightly soluble.
C. Na2CO3: Sodium carbonate (Na2CO3) falls under the category of soluble carbonates, as stated in the solubility rules. It is, therefore, not slightly soluble.
D. PbCl2: Lead chloride (PbCl2) is an exception to the solubility rule that most chloride salts are soluble. According to the rule, lead chloride is insoluble, making it slightly soluble in water.
So, the correct answer is D. PbCl2, as it is the only salt listed that is slightly soluble in water according to the solubility rules.