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Nataly [62]
2 years ago
10

If it requires 35.0 milliliters of 0.50 molar NaOH to neutralize 25.0 milliliters of HCl, what is the concentration of the HCl s

olution? (3 points)
Balanced equation: NaOH + HCl yields NaCl + H2O

Select one:
a. 0.36 M HCl
b. 0.70 M HCl
c. 1.1 M HCl
d. 1.4 M HCl
Chemistry
2 answers:
Over [174]2 years ago
8 0

Answer:

1.4

Explanation:

35 times .5 =25 times C. you have to get C by itself so you would have to do 35 times .5 and you get 17.5, than ÷ it by 25 and you get 1.4

victus00 [196]2 years ago
4 0

<u>Answer:</u>

<em>b. 0.70 M HCl is the Answer</em>

<em></em>

<u>Explanation:</u>

Molarity (M),  Molality (m), Normality (N),  Mass %,  Parts per million(ppm), billion(ppb), thousands(ppt)  are some of the terms we use to represent the concentration of the solution that is to represent the amount of solute present in a solvent.

The Balanced Chemical equation is :

NaOH + HCl > NaCl + H_2 O

Molarity is moles of solute present in 1L of the solution. The formula to find Molarity is

Molarity  = \frac {(moles solute)}{(volume of solution in L)} and its unit is mol/L

Rearranging the formula

We get                          

Moles = Molarity × Volume

Plugging in the values  

moles of NaOH=0.50M\times35mL (M=mol/L)

=0.50 mol/L \times 0.035L=0.0175 moles NaOH

Mole ratio of NaOH: HCl is 1:1  

So moles of NaOH = moles of HCl  = 0.0175moles

So,

Molarity  = \frac {(moles solute)}{(volume of solution in L)}

=\frac {0.0175mol}{25mL}\\\\=\frac {0.0175mol}{0.025L}\\\\=0.70M

(Answer)

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wariber [46]

Answer:

2.5 × 10² ppm

Explanation:

Step 1: Given data

  • Mass of NaCl: 0.050 g
  • Mass of the sample: 200. g

Step 2: Convert 0.050 g to μg

We will use the conversion factor 1 g = 10⁶ μg.

0.050 g × 10⁶ μg/1 g = 5.0 × 10⁴ μg

Step 3: Calculate the concentration of NaCl in ppm

The concentration of NaCl in ppm is equal to the micrograms of NaCl per gram of the sample.

5.0 × 10⁴ μg NaCl/200. g = 2.5 × 10² ppm

3 0
3 years ago
A solution of 0.0027 M K2CrO4 was diluted from 3.00 mL to 100. mL. What is the molarity of the new solution?
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Answer:

[K₂CrO₄] → 8.1×10⁻⁵ M

Explanation:

First of all, you may know that if you dilute, molarity must decrease.

In the first solution we need to calculate the mmoles:

M = mmol/mL

mL . M = mmol

0.0027 mmol/mL . 3mL = 0.0081 mmoles

These mmoles  of potassium chromate are in 3 mL but, it stays in 100 mL too.

New molarity is:

0.0081 mmoles / 100mL = 8.1×10⁻⁵ M

4 0
3 years ago
Given the following equilibrium constants: Kb B(aq) + H2O(l) ⇌ HB+(aq) + OH−(aq) 1/Kw H+(aq) + OH−(aq) ⇌ H2O(l) What is the equi
bija089 [108]

<u>Answer:</u> The value of K_c for the net reaction is \frac{K_b}{K_w}

<u>Explanation:</u>

The given chemical equations follows:

<u>Equation 1:</u>  B(aq.)+H_2O(l)\rightleftharpoons HB^+(aq.)+OH^-(aq.);K_b

<u>Equation 2:</u>  H^+(aq.)+OH^-(aq.)\rightleftharpoons H_2O(l);\frac{1}{K_w}

The net equation follows:

B(aq.)+H^+(aq.)\rightleftharpoons HB^+(aq.);K_c

As, the net reaction is the result of the addition of first equation and the second equation. So, the equilibrium constant for the net reaction will be the multiplication of first equilibrium constant and the second equilibrium constant.

The value of equilibrium constant for net reaction is:

K_c=K_1\times K_2

We are given:  

K_1=K_b

K_2=\frac{1}{K_w}

Putting values in above equation, we get:

K_c=K_b\times \frac{1}{K_w}=\frac{K_b}{K_w}

Hence, the value of K_c for the net reaction is \frac{K_b}{K_w}

7 0
3 years ago
The reaction A( g ) ⇌ 2 B( g ) A(g) ⇌ 2 B(g) has an equilibrium constant of K = 0.010 K = 0.010. What is the equilibrium constan
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Answer:

K = 10

Explanation:

Using Hess's law, it is possible to obtain the equilibrium constant, K, of a reaction using K of similar reactions. For example:

<em> If A ⇄ B K = X</em>

B ⇄ A K = 1/X

2A ⇄ 2B K = X².

Thus, if A(g) ⇄ 2B(g) K = 0.010

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B(g) ⇄ A(g) K = √100 = 10

<h3>K = 10</h3>
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