Hi. I'm not sure if my strategy for this problem is correct:
How many grams of CaCO3 will dissolve in 3.0x10^-2 mL of 0.050M Ca(NO3)2?
I think I'm supposed to convert molarity of Ca(NO3)2 into moles, but then i don't know how to get from mols of that to mols of CaCO3..is it a 1 to 1 ratio? from then on do i just convert to grams?
Thanks.
Well, well, well, aren't you feeling fancy with your chemistry problem!
To solve this, you're on the right track, my friend. Start by converting the volume of the Ca(NO3)2 solution to moles using its molarity. Once you have the moles of Ca(NO3)2, you can assume a 1:1 ratio between Ca(NO3)2 and CaCO3.
So, the number of moles of CaCO3 that will dissolve will be equal to the number of moles of Ca(NO3)2 you found.
To complete your journey, multiply the moles of CaCO3 by its molar mass to get the grams. Voilà! You did it!
But I have to warn you, don't clown around with the unit conversions and make sure your calculations are right. Otherwise, you might end up with a chemistry catastrophe!
Good luck, my word wizard of chemicals!
To determine the number of grams of CaCO3 that will dissolve in 3.0x10^-2 mL of 0.050M Ca(NO3)2, you are on the right track. Here is a step-by-step guide on how to approach this problem:
Step 1: Calculate the number of moles of Ca(NO3)2:
To convert the volume from mL to L, divide by 1000:
Volume = 3.0x10^-2 mL ÷ 1000 = 3.0x10^-5 L
Moles of Ca(NO3)2 = Molarity x Volume
Moles of Ca(NO3)2 = 0.050 mol/L x 3.0x10^-5 L = 1.5x10^-6 mol
Step 2: Determine the stoichiometry between Ca(NO3)2 and CaCO3:
The balanced equation for the dissolution of CaCO3 in water is:
Ca(NO3)2 + Na2CO3 -> CaCO3 + 2NaNO3
From the balanced equation, you can see that the ratio between Ca(NO3)2 and CaCO3 is 1:1.
Step 3: Calculate the number of moles of CaCO3:
Since the ratio is 1:1, the number of moles of CaCO3 is equal to the number of moles of Ca(NO3)2.
Therefore, there are 1.5x10^-6 moles of CaCO3 that will dissolve.
Step 4: Convert moles of CaCO3 to grams:
To convert moles to grams, you need to know the molar mass of CaCO3. The molar mass of CaCO3 is:
Calcium (Ca): 40.08 g/mol
Carbon (C): 12.01 g/mol
Oxygen (O): 16.00 g/mol (3 atoms)
Molar mass of CaCO3 = 40.08 g/mol + 12.01 g/mol + (16.00 g/mol x 3) = 100.09 g/mol
Now, calculate the grams of CaCO3:
Grams of CaCO3 = Moles of CaCO3 x Molar mass of CaCO3
Grams of CaCO3 = 1.5x10^-6 mol x 100.09 g/mol ≈ 1.50x10^-4 g
Therefore, approximately 1.50x10^-4 grams of CaCO3 will dissolve in 3.0x10^-2 mL of 0.050M Ca(NO3)2.
Hi there! I can definitely help you with that problem. Let's go through the steps together.
Step 1: Calculate the moles of Ca(NO3)2.
To do this, we can use the formula: moles = concentration (M) x volume (L).
In your case, the concentration of Ca(NO3)2 is given as 0.050 M, and the volume is given as 3.0x10^-2 mL. However, it's important to convert the volume to liters before using it in the equation. So, 3.0x10^-2 mL is equivalent to 3.0x10^-2/1000 L, which is 3.0x10^-5 L.
Now we can calculate the moles of Ca(NO3)2: moles = 0.050 M x 3.0x10^-5 L.
Step 2: Determine the moles of CaCO3.
The chemical equation for the dissolution of CaCO3 in water is: CaCO3(s) ⇌ Ca2+(aq) + CO32-(aq).
From this equation, we see that 1 mole of CaCO3 will dissociate into 1 mole of Ca2+ and 1 mole of CO32-.
Therefore, the moles of CaCO3 will be equal to the moles of Ca(NO3)2 from Step 1, assuming complete dissociation.
Step 3: Calculate the grams of CaCO3.
To convert moles of CaCO3 to grams, we need to use the molar mass of CaCO3. The molar mass is the sum of the atomic masses of each element in the compound. In this case, CaCO3 has a molar mass of 40.08 g/mol for Ca, 12.01 g/mol for C, and 16.00 g/mol for each O. Adding these together, the molar mass of CaCO3 is approximately 100.09 g/mol.
Now, to calculate the grams of CaCO3, you can use the formula: grams = moles x molar mass.
So, in summary, the correct approach is to first calculate the moles of Ca(NO3)2, then assume that it dissociates completely to give the same amount of moles of CaCO3, and finally convert the moles of CaCO3 to grams using the molar mass.
I hope this explanation helps! Let me know if you have any further questions.
This is a solubility product problem with CaCO3 in which there is a common ion (the Ca in Ca(NO3)2)
CaCO3 ==> Ca^+2 + CO3^=
Ksp = (Ca^+2)(CO3^=) = ??
Look up the Ksp for CaCO3.
Ca(NO3)2 ==> Ca^+2 + 2NO3^- (100% ionized)
[Ca(NO3)2] = 0.05 M
Let y = solubility of CaCO3, then y = concn of Ca^+2 from CaCO3 and y is concn of CO3^=. Total (Ca^+2) = y+0.05 (that's Ca from CaCO3 and Ca from Ca(NO3)2).
Solve for y, the units will be mols/L CaCO3, then convert from mols/L to mols/3.0 x 10^-2 mL, and from there to grams.
0.05 M = (Ca^+2) from Ca(NO3)2