Part 4 Key
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- Sep 2017
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chem.libretexts.org chem.libretexts.org
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If on the other hand, the ions are more attracted to the water, the leave the crystal and the compound is soluble.
So if the ion has a smaller charge than the water the compound is soluble?
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PbSO4(s)+2Na+(aq)+2ClO−4(aq)
Why would PbSO4 not be separated? Is this equation assuming that this is in an aqueous solution?
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Group 1A & Ammonium (the only cations in this list) b. NO3-, ClO4-, ClO3-, CH3CO2-
Can you go over these again tomorrow I'm still getting confused on finding which ones are soluble and which ones are not
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ClO4-
The equation says ClO subscript 3 with a negative charge. Is the answer key ClO subscript 4 with a negative a typo? The results are the same, but I'm just checking.
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When trying to predict if any (s) form from multiple solutions mixed together, draw a matrix and use the solubility rules to cancel out all the (aq).
When you write the equation do you write all of the one's that are precipitates on the right side of the arrow. How do you write the equation to this?
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Pure water does not conduct electricity, and it has been observed that when a substance dissolves in water, it may produce mobile ions that allow the water to conduct electricity, and we call that compound an electrolyte, or it may not, in which case we call it a nonelectrolyte.
For these water compounds to conduct electricity does there have to be an existing electrical current touching the water or will the compound create electricity when you mix one of these salts or acids with water? I hope this makes sense.
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BaCl2 (aq)
Same with these, they are aqueous, but why did we not mark them out?
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Ag2SO4 (aq)
Is there something different about this aqueous solution? Or should it be marked out as well?
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Quick 1'29" video
why would the aluminum and copper conduct with out water and NOT conduct while in water?
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Hg+2, Ca+2, Sr+2, Ba+2 & Pb+2
So these cations will make a bond soluble or insoluble?
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Ag+, Hg2+2, & Pb+2
So these cations will make a bond soluble or insoluble?
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amound
possible typo, amount dissolved?
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SO-4
possible typo sulfate = SO4(-2)
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which also means the hydronium ion concentration is higher than the hydroxide
Is the charge of the hydronium compound higher than the hydroxide compound as well?
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Acids and Bases
So for this section there is there a way for us to tell whether the acid/base are weak or strong?
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3.5: Acid-Base Reactions
Ok, so for this section, I think that I pretty well understand what it is that we are supposed to be doing, like looking at the reactions. But I am having trouble understanding how to know if an acid or a base is considered weak or strong. Is there a list that we are supposed to memorize? Or is there some sort of formula for figuring this out?
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chem.libretexts.org chem.libretexts.org
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Pb+2(aq)+ 2 NO3-(aq) + 2 Na+(aq)+ SO4-2(aq) 2 NO3-(aq)+ 2Na+(aq)+ PbSO4(s)
I am confused. There are ions on both sides of this equation, and I thought that the point was to eliminate those and only look at the reactive ions.
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chem.libretexts.org chem.libretexts.org
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6 NH4+(aq)
how did we go from 2 to 6 NH4+?
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H2O(l)
Are the other liquids that we should recognize? Are there rules for this like there is for solubility?
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BaI2+ H2SO4(aq)
Some sets (h. NaOH, i. BaI) is not labeled as s,g or aq, Do we use solubility rules for reactants if not labeled?
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3Mg+2
in the product - same ? about labeling ion as s, g, or aq?? same in k. Ca+2... I understand that the solid has no charge, but what state the ionic form?
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files.mtstatic.com files.mtstatic.com01
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Na3PO4
Where is the state here? (I chose aq because Na is a group 1a metal and should always be soluble?)
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Ca(CO3)2
carbonate has a -2 charge.
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chem.libretexts.org chem.libretexts.org
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Ag(s)
This is not balanced. There should be 2 Ag here.
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