Which type of molecule is shown below?

A solution containing 75.0 mL of 0.150 M strong acid (HCl) is titrated with 75.0 mL of 0.300 M strong base (NaOH). What is the p

Alborosie

Answer:

12.875

Explanation:

Balanced equation of the reaction:

HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)

mole of acid = mole of base

75 × 0.150 = volume of base needed × 0.3

volume of base needed = 37.5 ml

excess OH = 0.3 × 37.5 ml / 150 ml where total volume = 75 ml + 75 ml = 150 ml

excess OH = 0.075 M

pOH = - log (OH⁻) = - log (0.075 M) = 1.125

pH + pOH = 14

pH = 14 - pOH = 14 - 1.125 = 12.875

7 0

3 years ago

What is the difference between atomic mass and molar mass?

sweet-ann [11.9K]

Atomic mass is the mass of a chemical element expressed in atomic mass units. Molar mass the mass of a given substance divided by its amount of substance in (mol) .

6 0

4 years ago

Consider a 4 cation of Manganese. There are________ electrons accounted for in the noble gas of the shorthand electron configura

timurjin [86]

Answer: There are 18 electrons accounted for in the noble gas of the shorthand electron configuration. For the outermost electrons, there are 0 electrons in the 4s orbital and 3 electrons in the 3d orbitals.

Explanation:

Electronic configuration represents the total number of electrons that a neutral element contains. We add all the superscripts to know the number of electrons in an atom.

The electrons are filled according to Afbau's rule in order of increasing energies and thus the electronic configuration for Manganese with 25 electrons is :

$Mn:25:1s^22s^22p^63s^23p^64s^23d^5$

$Mn^{4+}:21:1s^22s^22p^63s^23p^63d^3$

$Mn^{4+}:21:[Ar]3d^3$

The nearest noble gas is Argon with 18 electrons.

There are 18 electrons accounted for in the noble gas of the shorthand electron configuration. For the outermost electrons, there are 0 electrons in the 4s orbital and 3 electrons in the 3d orbitals.

6 0

3 years ago

A certain material has a mass of 12.48 g while occupying 12.48 cm3 of space. What is this material?

Salsk061 [2.6K]

This material has a density of 1 g/cm3.
(since 12.48 g/ 12.48 cm3 = 1 g/cm3)

Therefore, this material is water.

5 0

3 years ago

Read 2 more answers

3NO2(g) + H2O(l) — 2HNO3(aq) + NO(g)

antiseptic1488 [7]

Answer:

A. 3.65 g of H2O.

B. 26.33 g of NO.

C. 7.53 g of HNO3.

Explanation:

The balanced equation for the reaction is given below:

3NO2(g) + H2O(l) —> 2HNO3(aq) + NO(g)

Next, we shall determine the masses of NO2 and H2O that reacted and the masses of HNO3 and NO produced from the balanced equation.

This is illustrated below:

Molar mass of NO2 = 14 + (16x2) = 46 g/mol

Mass of NO2 from the balanced equation = 3 x 46 = 138 g

Molar mass of H2O = (2x1) + 16 = 18 g/mol

Mass of H2O from the balanced equation = 1 x 18 = 18 g

Molar mass of HNO3 = 1 + 14 + (16x3) = 63 g/mol

Mass of HNO3 from the balanced equation = 2 x 63 = 126 g.

Molar mass of NO = 14 + 16 = 30 g/mol

Mass of NO from the balanced equation = 1 x 30 = 30 g.

Summary:

From the balanced equation above,

138g of NO2 reacted with 18 g of H2O to produce 126 g of HNO3 and 30 g of NO.

A. Determination of the mass of H2O required to react with 28.0 g

of NO2.

This is illustrated below:

From the balanced equation above,

138g of NO2 reacted with 18 g of H2O.

Therefore, 28 g if NO2 will react with = (28 x 18)/138 = 3.65 g of H2O.

Therefore, 3.65 g of H2O is needed for the reaction.

B. Determination of the mass of NO produced from 15.8 g of H2O.

This is illustrated below:

From the balanced equation above,

18 g of H2O reacted to produce 30 g of NO.

Therefore, 15.8 g of H2O will react to produce = (15.8 x 30)/18 = 26.33 g of NO.

Therefore, 26.33 g of NO were produced from the reaction.

C. Determination of the mass of HNO3 produced from 8.25 g of NO2.

This is illustrated below:

From the balanced equation above,

138g of NO2 reacted to produce 126 g of HNO3.

Therefore, 8.25 g of NO2 will react to produce = (8.25 x 126)/138 = 7.53 g of HNO3.

Therefore, 7.53 g of HNO3 were produced from the reaction.

7 0

3 years ago