Shay K. answered • 05/31/19
CS Student with experience as a professional software developer
Alright, so let's first break this down into moles. Molarity is (moles of solute)/(liters of solution).
HCL(aq) (0.525 L)(0.80 mol/L) = 0.420 mol of HCL
Sr(OH)2(aq) (0.315 L)(X mol/L) = Y mol of Sr(OH)2(aq)
We are trying to find X, the molarity of Sr(OH)2(aq). Since we already know how much we have (0.315 liters) we just need to figure out how many moles of Sr(OH)2(aq) are used to neutralize our 0.420 mol of HCl, what is noted as our Y value. So, let's take apart this acid and base.
HCl is an acid comprised of two ions, H+ and Cl-. Sr(OH)2 is a base made up of OH- and Sr2+. We can balance this equation as follows
2 H+ + 2 Cl- + 2 OH- + Sr2+ -> 2 H2O + SrCl2
We can see that 1 mol of Sr(OH)2 can neutralize 2 mol of HCl. With this, we can calculate the number of mol of Sr(OH)2 which we denoted as variable Y above.
Y = (0.420 mol HCl)(1 mol Sr(OH)2 / 2 mol HCL) = 0.210 mol Sr(OH)2
Now, we plug that back into our initial equation and solve for X.
Sr(OH)2(aq) (0.315 L)(X mol/L) = 0.210 mol of Sr(OH)2(aq)
X = 0.667 mol of Sr(OH)2(aq) / L = 0.667 M Sr(OH)2(aq)
Shay K.
The balanced equation is 2 HCl + Sr(OH)2 -> 2 H2O + SrCl2 In my answer above, I separated the ions on the reactant side (left side) of the equation.05/31/19
Elliot C.
You are a lifesaver do you do tutoring and what are the states of the 2H20 +SrCL2 like g s or or aq05/31/19
Shay K.
I do tutoring, but I am not approved by Wyzant, yet. However, I periodically go on ask an expert. You're welcome to check back on my profile when Wyzant has approved me, and I have a microphone/camera setup so I can do online tutoring for you. H2O is water, so it's a liquid (l) SrCl2 is soluble in water, if you follow the solubility rules. So it's (aq) because the solution is comprised of only H2O and SrCl2.05/31/19
Elliot C.
Hey can you check out the new question I posted where can I contact you for tutoring?05/31/19
Elliot C.
What is the balanced equation for this?05/31/19