I don't understand how to do this problem.
You mix 1.00 L of 2.00 M BaCl2 with 1.00 L of 2.00 M AgNO3. What compounds remain in the solution, and what are their concentrations?
BaCl2 + 2AgNO3 ---> 2AgCl + Ba(NO3)2
Is it trying to trick me with the two sets of information?
I don't think so. It's a limiting reagent problem, more or less like the last one you worked, and posted your answer. The AgCl, you realize, is a ppt.
I'm confused.. Could you help me work it out?
Oh never mind I think i've got it.
Oh. nope. lost again. I don't understand what I'm doing. My book says the answer is .50 M Ba(NO3)2 but I'm not getting that.
See your post above.
No, the problem is not trying to trick you with the two sets of information. It's giving you the initial information about the compounds and their concentrations to set up the chemical reaction. The reaction equation is balanced and shows the stoichiometry of the reactants and products.
To solve the problem, you need to follow these steps:
1. Determine the limiting reagent: Compare the molar ratios of the reactants in the balanced equation to determine which one will be completely consumed. In this case, the molar ratio between BaCl2 and AgNO3 is 1:2, which means that 1 mole of BaCl2 reacts with 2 moles of AgNO3. Since the concentrations of BaCl2 and AgNO3 are the same, you have an equal amount of moles for both. Therefore, you have an excess of both reagents, and no reaction will occur to completion.
2. Determine the products formed: Although no reaction will go to completion, you can determine the products that will form based on the balanced equation. The products are 2 moles of AgCl and 1 mole of Ba(NO3)2.
3. Calculate the concentrations of the remaining compounds: Since there is no reaction to completion, the remaining compounds will still be in the solution. Their concentrations will be the same as the initial concentrations. Therefore, the remaining compounds are BaCl2 and AgNO3, and their concentrations are both 2.00 M.
In summary, the compounds that remain in the solution after the reaction are BaCl2 and AgNO3, and their concentrations remain at 2.00 M.