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givi [52]
2 years ago
10

In an acid-base neutralization reaction 43.74 ml of 0.500 m potassium hydroxide reacts with 50.00 ml of sulfuric acid solution.

what is the concentration of the h2so4 solution?'
Chemistry
2 answers:
timama [110]2 years ago
7 0
The   neutralization reaction between  potassium  hydroxide  and  sulfuric  acid   is  as  follows
2KOH  +  H2SO4 ---> K2SO4  +  2H2O

number  of   moles  of  KOH=  (43.74  x  0.500)/  1000=  0.02187 moles

the  reacting ratio  of  KOH  to H2SO4  is  2:1  therefore  the   moles  of  H2SO4  is  =  0.021187/2=  0.01094 moles

concentration(molarity) = ( 0.01094/50 ) x 1000=  0.2188M
Orlov [11]2 years ago
3 0

<u>Answer:</u> The concentration of sulfuric acid is 0.219 M

<u>Explanation:</u>

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is H_2SO_4

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is KOH.

We are given:

n_1=2\\M_1=?M\\V_1=50.00mL\\n_2=1\\M_2=0.500M\\V_2=43.74mL

Putting values in above equation, we get:

2\times M_1\times 50.00=1\times 0.500\times 43.74\\\\M_1=\frac{1\times 0.500\times 43.74}{2\times 50.00}=0.219M

Hence, the concentration of sulfuric acid is 0.219 M

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A graduated cylinder holds 100 mL of water. A lead weight is dropped into the cylinder bringing the new volume up to 450 mL. If
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11.43g/mL

Explanation:

Given parameters:

Volume of water in the graduated cylinder = 100mL

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Mass of lead weight = 4000g

Unknown:

Density of the lead weight = ?

Solution:

Density is the mass per unit volume of a body.

  Density  = \frac{mass}{volume}

Volume of the lead weight = volume of water displaced

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Density = \frac{4000}{350}  = 11.43g/mL

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2 years ago
Movement of the ___<br> creates the London dispersion forces.
Tanzania [10]

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Which is stronger, the strong force (SF) or the electromagnetic force (EMF)? Describe how they battle each other in the nucleus.
Roman55 [17]

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2 years ago
A gas occupies a volume at 34.2 mL at a temperature of 15.0 C and a pressure of 800.0 torr. What will be the volume of this gas
Grace [21]
The answer is 34.1 mL.
Solution:
Assuming ideal behavior of gases, we can use the universal gas law equation
     P1V1/T1 = P2V2/T2
The terms with subscripts of one represent the given initial values while for terms with subscripts of two represent the standard states which is the final condition.
At STP, P2 is 760.0torr and T2 is 0°C or 273.15K. Substituting the values to the ideal gas expression, we can now calculate for the volume V2 of the gas at STP:
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3 0
2 years ago
Read 2 more answers
A 0.15 m solution of chloroacetic acid has a ph of 1.86. What is the value of ka for this acid?
dem82 [27]

Answer: 1.67\times 10^{-3}

Explanation:

ClCH_2COOH\rightarrow ClCH_2COO^-+H^+

   cM              0             0

c-c\alpha        c\alpha          c\alpha  

So dissociation constant will be:

K_a=\frac{(c\alpha)^{2}}{c-c\alpha}

Given:  c = 0.15 M

pH = 1.86

K_a = ?

Putting in the values we get:

Also pH=-log[H^+]

1.86=-log[H^+]

[H^+]=0.01

[H^+]=c\times \alpha

0.01=0.15\times \alpha

\alpha=0.06

As [H^+]=[ClCH_2COO^-]=0.01

K_a=\frac{(0.01)^2}{(0.15-0.15\times 0.06)}

K_a=1.67\times 10^{-3]

Thus the vale of K_a for the acid is 1.67\times 10^{-3}

4 0
2 years ago
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