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muminat
3 years ago
5

How many milliliters of .085 m naoh are required to titrate 25 ml of .072 m hbr to the equivalence point?

Chemistry
1 answer:
SOVA2 [1]3 years ago
8 0
The ML  of 0.85  m NaOH    required   to  titrate  25 ml of  0.72m hbr  to  the  equivalence  point  is calculated  as  follows

calculate  the moles  of HBr used

moles  = molarity  x  volume

25  x0.072/1000=  0.0018 moles


write the  equation  for  reaction

NaOH + HBr = NaBr  +  H2O
from   reacting   equation the  mole ratio  between  NaOH  to  HBr  is  1:1  therefore  the  moles of  NaOH  =  0.0018 moles

volume   =  moles/molarity
0.0018/0.085 =  0.021  L  in Ml  =  0.021  x1000=21.18 Ml  ofNaOH

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Answer :

(a) The heat released by the metal is -312.48 J

(b) The specific heat of the metal is 0.0944J/g^oC

Explanation :

<u>For part A :</u>

Heat released by the metal = Heat absorbed by the calorimeter + Heat absorbed by the water

q=[q_1+q_2]

q=[c_1\times \Delta T+m_2\times c_2\times \Delta T]

where,

q = heat released by the metal

q_1 = heat absorbed by the calorimeter

q_2 = heat absorbed by the water

c_1 = specific heat of calorimeter = 51.5J/^oC

c_2 = specific heat of water = 4.184J/g^oC

m_2 = mass of water = 50.0 g

\Delta T = change in temperature = (T_{final}-T_{initial})=23.2-22.0=1.2^oC

Now put all the given values in the above formula, we get:

q=[(51.5J/^oC\times 1.2^oC)+(50.0g\times 4.184J/g^oC\times 1.2^oC)]

q=312.48J

Thus, the heat released by the metal is -312.48 J

<u>For part B :</u>

q=m\times c\times \Delta T

q = heat released by the metal = -312.48 J

m = mass of metal = 43.1 g

c = specific heat of metal = ?

\Delta T = change in temperature = (T_{final}-T_{initial})=23.2-100=76.8^oC

Now put all the given values in the above formula, we get:

-312.48J=43.1g\times c\times 76.8^oC

c=0.0944J/g^oC

Thus, the specific heat of the metal is 0.0944J/g^oC

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When one evaporates a pure substance, what would be seen after this evaporation?
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A 500.0 g block of dry ice (solid CO2, molar mass = 44.0 g) vaporizes at room temperature. Calculate the volume of gas produced
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Considering the ideal gas law, the volume of gas produced at 25.0 °C and 1.50 atm is 184.899 L.

<h3>Definition of ideal gas</h3>

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

<h3>Ideal gas law</h3>

An ideal gas is characterized by absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of gases:

P×V = n×R×T

<h3>Volume of gas</h3>

In this case, you know:

  • P= 1.50 atm
  • V= ?
  • n= 500 g×\frac{1 mole}{44 g}= 11.36 moles, being 44 \frac{g}{mole} the molar mass of CO₂
  • R= 0.082 \frac{atmL}{molK}
  • T= 25 C= 298 K (being 0 C=273 K)

Replacing in the ideal gas law:

1.50 atm×V = 11.36 moles×0.082\frac{atmL}{molK} × 298 K

Solving:

V= (11.36 moles×0.082\frac{atmL}{molK} × 298 K) ÷ 1.50 atm

<u><em>V= 184.899 L</em></u>

Finally, the volume of gas produced at 25.0 °C and 1.50 atm is 184.899 L.

Learn more about the ideal gas law:

<u>brainly.com/question/4147359?referrer=searchResults</u>

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