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natali 33 [55]
3 years ago
12

47.0ml of a HBr solution were titrated with 37.5ml of a 0.215M LiOH solution to reach the equivalence point. what is the molarit

y of the HBr solution
Chemistry
1 answer:
faltersainse [42]3 years ago
4 0

Hello!

The molarity of the HBr solution is 0,172 M.

Why?

The neutralization reaction between LiOH and HBr is the following:

HBr(aq) + LiOH(aq) → LiBr(aq) + H₂O(l)

To solve this exercise, we are going to apply the common titration equation:

M1*V1=M2*V2

M1=\frac{M2*V2}{V1}= \frac{0,215 M * 37,5 mL}{47 mL}=0,172 M

Have a nice day!

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Answer:

Beta decay

Explanation:

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6 0
1 year ago
Consider the following generic reaction for which Kp = 5.51 × 105 at 25°C:2R(g)+A(g)⇌2Z(g)What is the value of Kc for the reacti
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Answer:

Kc = 1.35x10^7

Explanation:

Let's write the reaction again:

2R + A <------> 2Z    Kp = 5.51x10^5

In order to know the value of Kc, we need to write the expression that relations the Kp with Kc which is:

Kp = Kc * (RT)^Δn (1)

Where:

R: 0.082 L atm/ K mol

Δn: difference between the coefficients of the reaction

Kc: equilibrium constant

T: temperature in K

Now, from the equation (1) we can solve for Kc:

Kc = Kp / (RT)^Δn (2)

Now, before do any calculations, let's do first the value of Δn:

Δn = 2 - (2+1) = -1

Now, replacing all values in (2):

Kc = 5.51x10^5 / (0.082*298)^-1

Kc = 1.346x10^7

The third option is the correct one.

7 0
3 years ago
What is the pH of a solution after the addition of 30.0 mL of 0.100 M NaOH to 50.0 mL of 0.10 M HBr?
Pani-rosa [81]

Answer:

pH = 1.6

Explanation:

  • HBr + NaOH ⇒ NaBr + H2O

0 mL NaOH:

  • HBr ↔ H3O+  +  Br-

⇒ [ H3O+] = M HBr = 0.1 M

⇒pH = -log [H3O+] = 1

30 mL NaOH:

⇒ mol NaOH = 0.1 mol / L * 0.03 L =  3 E-3 mol

⇒ mol HBr = 0.05 L * 0.1 mol/L = 5 E-3 mol

⇒ M HBr = ( 5 E-3 mol - 3 E-3 mol) / 0.08 L = 0.025 M

⇒ pH = - log (0.025) = 1.6

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3 years ago
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but where Is the volume in order for us to determine the concentration. since we have moles in H+ ions

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