molar mass of NaCl-58.5g so B)1.00 mol
Ca=40g
P=31g
Ca3=120g
P2=62g
Ca3P2=182g
Ca3/Ca3p2=120/182=0.6593=approximately 65.93%
The pH at the equivalence point always not equal to 7 in a neutralization titration when titration occur between weak acid and weak base , strong acid and weak base or strong base weak acid. The reason behind it is given as,
- At equivalence point the product is present by reacting from acid and base.
- So, when weak acid titrate with strong base then the solution will be weak base at equivalence point.
When strong acid is neutralize with strong base then it form neutral product at the equivalence point. Hence the final conclusion is that the pH of the solution in which titration is takes place between strong acid and strong base is 7 that is neutral left titration between all type of acids and bases ha pH not equal to 7 .
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Answer:
P2 = 2.25 atm
Explanation:
Given:
V1 = 1.5 L. V2 = 2.0 L
P1 = 3.0 atm. P2 = ?
Use Boyle's law and solve for P2:
P1V1 = P2V2
or
P2 = (V1/V2)P1
= (1.5 L/2.0L)(3.0 atm)
= 2.25 atm
<u>Answer:</u> The number of moles of ammonium nitrate is 0.004 moles.
<u>Explanation:</u>
To calculate the number of moles for given molarity, we use the equation:
We are given:
Molarity of 
solution = 0.125 M
Volume of solution = 32.5 mL
Putting values in above equation, we get:
Hence, the number of moles of ammonium nitrate is 0.004 moles.
