QUESTION 6

What's the specific heat of water?

natita [175]

it is over 32 degrees Fahrenheit (freezing), and below 120 degrees Fahrenheit (boiling)

8 0

3 years ago

Read 2 more answers

A sample of nitric acid contains both H3O ions and NO3 ions. This sample has a pH

bearhunter [10]

Answer : The name of positive ion present in this sample is, hydronium ion.

Explanation :

For formation of a neutral ionic compound, the charges on cation and anion must be balanced.

The cation is formed by loss of electrons by metals and anions are formed by gain of electrons by non metals.

Ion : An ion is formed when an atom looses or gains electron.

When an atom looses electrons, it will form a positive ion known as cation.

When an atom gains electrons, it will form a negative ion known as anion.

As per question, hydronium ion or hydrogen ion is having an oxidation state of +1 called as $H_3O^{+}$ or $H^+$ cation and nitrate ion $NO_3^{-}$ is an anion with oxidation state of -1.

Thus they combine and their oxidation states are exchanged and written in simplest whole number ratios to give neutral $HNO_3$ .

Hence, the name of positive ion present in this sample is, hydronium ion.

4 0

4 years ago

What is the mistake in the set up above?<br>

Misha Larkins [42]

Answer:

Explanation:

d

7 0

3 years ago

In what area of the titration curve for phosphoric acid (h3po4) is the molecule fully deprotonated?

Arada [10]

The titration curve should have flat regions centered around each of the

three halfway points (buffer zones) and sharp increases in pH around the

equivalence points.

Initial pH

This is determined by the most acidic of the Ka values and the initial

concentration of the acid. (Same as a monoprotic acid)

Half-way points

At each halfway point, the pH = pKa of the group you are titrating. At this point in

the titration curve, we are in a buffering region, and the curve will be relatively

flat.

Equivalence points

At each equivalence point, the pH is the average of the pKa values above and

below. At the last equivalence point (the endpoint), the pH is determined by the

Kb of the conjugate base of the weakest acid.

Plotting the titration of 100 mL of 0.10 M phosphoric acid with 1.0 M NaOH.

H3PO4 + H2O  H2PO4

-

+ H3O+

Ka1 = 7.5 x 10-3

H2PO4

-

+ H2O  HPO4

2- + H3O+

Ka2 = 6.2 x 10-8

HPO4

2- + H2O  PO4

3- + H3O+

Ka3 = 4.2 x 10-13

Plot these points and connect them to determine the titration curve of phosphoric acid. The curve should be relatively flat around each of the halfway points when we are in a buffering region.

The titration curve should have flat regions centered around each of the

three halfway points (buffer zones) and sharp increases in pH around the

equivalence points.

For more information on the titration curve click on the link below:

brainly.com/question/3130161

#SPJ4

4 0

2 years ago

How much heat energy is needed to heat 250 g of water from 200C to its boiling point and then completely vaporize it?

alexandr1967 [171]

Answer: 40.66kJ/mol.

Explanation:Assuming that pressure is equal to Explanation:Assuming that pressure is equal to 1 atm Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at 100

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at 100∘

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at 100∘C

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at 100∘C .

Explanation:Assuming that pressure is equal to 1 atm , boiling water at its boiling point implies providing it with enough heat to turn it from liquid at 100∘C to vapor at 100∘C .The amount of heat needed to allow one mole of water to undergo this phase change is called the enthalpy change of vaporization,

nge of vaporization, Δ

nge of vaporization, ΔH

nge of vaporization, ΔHvap

nge of vaporization, ΔHvap .

nge of vaporization, ΔHvap .For water at

nge of vaporization, ΔHvap .For water at 100

nge of vaporization, ΔHvap .For water at 100∘

nge of vaporization, ΔHvap .For water at 100∘C

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal to

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal toΔ

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal toΔH

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal toΔHvap

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal toΔHvap=

nge of vaporization, ΔHvap .For water at 100∘C , the enthalpy change of vaporization is equal toΔHvap=40.66 kJ/mol

8 0

3 years ago