What is the molarity of a solution made by mixing 75.0 mL of 3.00 M NH₄OH with enough water to give 250. mL of solution?

Please explain and show work.

Answer:

Frequency and wavelength are inversely proportional. c=f⋅λ (The speed of light is directly proportional to f and λ)

Answer:

[tex]C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-[/tex]

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to figure out the required net ionic equation by firstly writing out the complete molecular equation between aspirin and sodium acetate:

[tex]C_9H_8O_4+NaC_2H_3O_2\rightarrow C_2H_4O_2+NaC_9H_7O_4[/tex]

Whereas acetic acid and sodium acetylsalicylate are formed. Now, we write the complete ionic equation whereby sodium acetate and sodium acetylsalicylate are ionized because they are salts yet neither aspirin nor acetic acid are ionized as they are weak acids:

[tex]C_9H_8O_4+Na^++C_2H_3O_2^-\rightarrow C_2H_4O_2+Na^++C_9H_7O_4^-[/tex]

Finally, for the net ionic equation we cancel out the sodium spectator ions to obtain:

[tex]C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-[/tex]

Regards!

Answer:

Explanation:

maleic acid ⇒ fumaric acid

ΔHreaction = ΔHproduct - ΔHreactant

ΔHproduct = -1336.0 kJ mol⁻¹

ΔHreactant = - 1359.2 kJ mol⁻¹.

ΔHreaction = -1336.0 kJ mol⁻¹ - ( - 1359.2 kJ mol⁻¹.)

=   1359.2 kJ mol⁻¹   -1336.0 kJ mol⁻¹

= 23.2 kJ mol⁻¹ .

Enthalpy of isomerization from maleic to fumaric acid is 23.2 kJ per mol.

Answer:

B

Explanation:

Answer:

a) [tex]K_{2} S[/tex] and [tex]NH_{4} Cl[/tex] :

There are no insoluble precipitate forms.

b) [tex]Ca Cl_{2}[/tex] and [tex](NH_{4} )_{2} Co_{3}[/tex] :

There are the insoluble precipitates of [tex]CaCo_{3}[/tex]  forms.

c) [tex]Li_{2}S[/tex] and [tex]MnBr_{2}[/tex] :

There are the insoluble precipitates of [tex]MnS[/tex]  forms.

d) [tex]Ba(No_{3} )_{2}[/tex] and [tex]Ag_{2} So_{4}[/tex] :                        

As [tex]Ag_{2} So_{4}[/tex] is insoluble, therefore no precipitate forms.

e) [tex]Rb_{2}Co_{3}[/tex] and [tex]NaCl[/tex]:

There are no insoluble precipitates forms.

Explanation:

a)

Solubility rule suggests:- [tex]K_{2} S[/tex] ⇒ soluble, [tex]NH_{4} Cl[/tex] ⇒ soluble.

                                          KCl ⇒ soluble, [tex](NH_{4})_{2} S[/tex]  ⇒ soluble.

There are no insoluble precipitate forms.

b)

Solubility rule suggests:- [tex]Ca Cl_{2}[/tex] ⇒ soluble, [tex](NH_{4} )_{2} Co_{3}[/tex] ⇒ soluble.

                                        [tex]CaCo_{3}[/tex] ⇒ insoluble, [tex]NH_{4} Cl[/tex]  ⇒ soluble.

There are the insoluble precipitates of [tex]CaCo_{3}[/tex]  forms.

c)

Solubility rule suggests:- [tex]Li_{2}S[/tex] ⇒ soluble, [tex]MnBr_{2}[/tex] ⇒ soluble.

                                        [tex]LiBr[/tex] ⇒ soluble, [tex]MnS[/tex]  ⇒ insoluble.

There are the insoluble precipitates of [tex]MnS[/tex]  forms.

d)

Solubility rule suggests:- [tex]Ba(No_{3} )_{2}[/tex] ⇒ soluble, [tex]Ag_{2} So_{4}[/tex] ⇒insoluble.

As [tex]Ag_{2} So_{4}[/tex] is insoluble, therefore no precipitate forms.

e)

Solubility rule suggests:- [tex]Rb_{2}Co_{3}[/tex] ⇒ soluble, [tex]NaCl[/tex] ⇒ soluble.

                                        [tex]RbCl[/tex] ⇒ soluble, [tex]Na_{2} Co_{3}[/tex]  ⇒ soluble.

There are no insoluble precipitates forms.

Answer:

[tex]K=1.7x10^{-3}[/tex]

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to solve this problem by firstly setting up the equilibrium expression for the given reaction, in agreement to the law of mass action:

[tex]K=\frac{[NO]^2}{[N_2][O_2]}[/tex]

Next, we plug in the given concentrations on the data table to obtain:

[tex]K=\frac{(0.034)^2}{(0.69)(0.98)}\\\\K=1.7x10^{-3}[/tex]

Regards!

Answer:

6.4 L

Explanation:

As the temperature and pressure are assumed to remain the same, we can solve this problem by using Avogadro's law, which states:

Where in this case:

We input the data given by the problem:

And solve for V₂:

Answer:

Increase

Decrease

Explanation:While in solution, ionic substances produce ions. The ions in solution determine the conductivity of the solution.

The ionic strength of a solution shows the concentration of ions in a given solution. The more the number of ions in the solution, the greater the ionic strength of the solution and vice versa.

When HNO3 is added to a solution of KOH, the number of ions in the solution increases and so does the ionic strength of the solution.

When KOH is added to a solution of CaCl2 then Ca(OH)2 is formed. The formation of a solid precipitate decreases the concentration of ions in solution as well as the ionic strength of the solution.

Answer:

4.858 g

Explanation:

Start with the formula

density = [tex]\frac{mass}{volume}[/tex]

density = 1.98 g/mL

volume = 2.45 mL

mass = ??

rearrange the formula to solve for mass

(density) x (volume) = mass

Add in the substitutes and solve for mass

1.98 g/mL x 2.45 mL = 4.858 g

The volume of 1.5 moles of gas at STP  is 33.6 L.

The volume of the gas at STP is calculated as follows;

I mole of gas at STP = 22.4 L

1.5 moles of the gas at STP = ?

= 1.5 moles  x 22.4 L/mole

= 33.6 L

Thus, the volume of 1.5 moles of gas at STP  is 33.6 L.

Learn more about volume of gas here: https://brainly.com/question/27100414

#SPJ1

Answer:

77%

Explanation:

First we convert 3.0 g of cyclohexanol (C₆H₁₂O) to moles, using its molar mass:

Then we convert 1.9 g of cyclohexene (C₆H₁₀) to moles, using its molar mass:

Finally we calculate the theoretical yield:

this is the difference between organic and inorganic if this doesn't help you can research more on it

The properties of solids, liquids and gases regarding their shapes and volumes are:

                       Shape             Volume

Solids              Fixed                Fixed

Liquids           Variable            Fixed

Gases             Variable           Variable

Solids have strong attraction forces between their molecules. Thus, the molecules are closely packed with little movement. As a consequence, both shape and volume are fixed.

In liquids, attraction and repulsion forces are similar. They have a little more movement than the solid state. Then, they do have a fixed volume but they adopt the shape of the container.

Gases have very weak attraction forces between their molecules. They move very freely and expand trying to occupy as much volume as possible. So, they have a variable volume and shape (adopt the shape of the container).

You can learn more about states of matter here:

https://brainly.com/question/18538345

Answer:

Milli, m.

Explanation:

Hey there!

In this case, according to the given information, it turns out possible for us to answer to this question by bearing to mind the attached file whereas the most common prefixes and their factors are shown both in standard and scientific notation.

In such a way, we will be able to infer that the prefix related to the numerical value of 0.001 is milli, m, for example 1 mm which is 0.001 m.

Regards!

Answer:

See explanation

Explanation:

Truly, the second law of thermodynamics requires that spontaneous processes generate entropy, either in the system or in the surroundings.

When a solid is dissolved in a liquid, the solid dissociates into ions. These ions increases the number of particles and hence the entropy of the system thereby making the process spontaneous.

Hence, the dissolution of a substance via an endothermic process is spontaneous because of increase in the number of particles which in turn increases the entropy of the system.

Answer:

From least polar covalent to most polar covalent;

S-I< Br-Cl < N-H< Te-O

From most ionic to least ionic

Cs-F> Sr-Cl> Li- N> Al-O

Explanation:

Electro negativity is the ability of an atom in a bonding situation to attract the electron pair of a bond towards itself.

Electro negativity difference between two atoms determines the nature of bond existing between any two atoms. When this difference is large, an ionic bond exists in the compound. However, an intermediate difference in electro negativity implies the existence of a polar covalent bond.

Hence, going by electro negativity differences as mentioned in the question, the bonds in the answer were arranged in order of increasing polar covalent nature or decreasing ionic nature as shown.

Answer:

The molar heat of fusion for a given substance basically tells you how much heat is required to melt one mole of that substance at its melting point from two angles.

Explanation:

:)

Answer:

CO2 is a trigonal planar.

Answer:

C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g)

Explanation:

The chemical formula of propane is C₃H₈. When it burns in air, it reacts with gaseous oxygen (O₂), so carbon dioxide (CO₂) and water (H₂O) are formed. The combustion reaction is the following:

C₃H₈(g) + O₂(g) → CO₂(g) + H₂O(g)

Finally, we have to balance the equation. For this, we write a coefficient 3 in CO₂, then a coefficient 4 in H₂O, and a coefficient 5 in O₂. We obtain the balanced equation:

C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g)

Explanation:

the reaction is a decomposition reaction since potassium hypochlorite is decomposed into potassium chloride and oxygen

Answer:

84.27 g

Explanation:

How many grams of hydrogen are in 10.45 moles of C₃H₈?

Step 1: Calculate the moles of atoms of hydrogen

The molar ratio of C₃H₈ to H is 1:8.

10.45 mol C₃H₈ × 8 mol H/ 1mol C₃H₈ = 83.60 mol H

Step 2: Calculate the mass corresponding to 83.60 moles of hydrogen

The molar mass of hydrogen is 1.008 g/mol.

83.60 mol × 1.008 g/mol = 84.27 g

Answer:

c. C3H9N2O2

Explanation:

The empirical formula of a compound is defined as the simplest whole number ratio of atoms present in a molecule. To solve this question we need to convert the mass of each atom to moles. With the moles we can find the ratio as follows:

Moles N -Molar mass: 14.01g/mol-

0.420g N * (1mol/14.01g) = 0.0300 moles N

Moles O -Molar mass: 16g/mol-

0.480g O * (1mol/16g) = 0.0300 moles O

Moles C -Molar mass: 12.01g/mol-

0.540g C * (1mol/12.01g) = 0.0450 moles C

Moles H -Molar mass: 1.0g/mol-

0.135g H * (1mol/1g) = 0.135moles H

Dividing in the moles of N (Lower number of moles) the ratio of atoms is:

N = 0.0300 moles N / 0.0300 moles N = 1

O = 0.0300 moles O / 0.0300 moles N = 1

C = 0.0450 moles C / 0.0300 moles N = 1.5

H = 0.135 moles H / 0.0300 moles N = 4.5

As the empirical formula requires whole numbers, multiplying each ratio twice:

N = 2, O = 2, C = 3 and H = 9

And the empirical formula is:

Answer:

If 13.50 mL of an aluminum chloride solution is needed to reach the equivalence point with 10.00 mL of 0.109 M silver nitrate solution, determine the molarity of the aluminum chloride solution.

Explanation:

The balanced chemical equation of the reaction is:

[tex]AlCl_3(aq)+3AgNO_3(aq)->3AgCl(s)+Al(NO_3)_3(aq)[/tex]

So, one mole of aluminum chloride reacts with three moles of silver nitrate.

At the equivalence point,

the number of moles of each reactant must be equal.

The number of moles = molarity x volume in L.

Number of moles of AlCl3 = volume x molarity

=0.0135Lx Molarity

The number of moles of AgNO3 = 3 x 0.010Lx 0.109M

Thus,

0.0135Lx Molarity = 3 x 0.010Lx 0.109M

Molarity of AlCl3 :

[tex]Molarity of Alcl_3=3 x 0.010Lx 0.109M/0.0135\\=0.242M[/tex]

Answer is : 0.242M.

Answer:

It has no fixed shape and therefore takes the shape of the part of the container in which it is placed

Explanation:

here's the answer to your question

Answer:

The heat absorbed in Trial 2 is about 1,240 J greater than the heat absorbed in Trial 1.

The heat absorbed in Trial 2 is about 1,674 J greater than the heat absorbed in Trial 1.

The amount of heat absorbed or released by a substance can be calculated using the formula Q = mcΔT, where Q represents heat, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, the mass (m) is the same in both trials, but the initial and final temperatures (ΔT) differ. By comparing the values of ΔT in both trials, we can determine the difference in the amount of heat absorbed.

In Trial 1, the initial temperature is 15.0 °C and the final temperature is 65.0 °C, resulting in a ΔT of 65.0 - 15.0 = 50.0 °C.

In Trial 2, the initial temperature is 10.0 °C and the final temperature is 65.0 °C, resulting in a ΔT of 65.0 - 10.0 = 55.0 °C.

Since the specific heat capacity of water is approximately 4.18 J/g°C, we can calculate the difference in heat absorbed:

ΔQ = mcΔT = (80.0 g)(4.18 J/g°C)(55.0 °C - 50.0 °C) = 1,674 J

Therefore, the heat absorbed in Trial 2 is approximately 1,674 J greater than the heat absorbed in Trial 1.

To learn more about  specific heat capacity,  here

https://brainly.com/question/29766819

#SPJ2

Answer:

0.60 mol

Explanation:

The equation is as stated below;

2 C2H2 + 5 O2----> 4 CO2 +2 H2O

5 mole amount of Oxygen produces 2 mole of water. Then upon reaction of 1.5mol of O2.

thus, number of mole = (1.5*2)/5 =0.60mol

Answer:

Explanation:

Well, obviously a molecule with polar bonds can be polar in itself. It's like saying I am an atheltic person who can just reach the basketball rim with my head and also I can dunk.

But if the question is how can a molecule that in non-polar have polar bonds, well, its because the polar bonds' dipole cancels each other out. It's like a tight rope. If a person pulls in one direction, it intuitively, the rope would go in that direction. However, if a person pulls in the other direction with the same amount of force, the rope stays still. This is the same case. Although molecules can have different electronegativities, the pull of electrons in one direction is cancelled out by a pull in the opposite direction, making the net dipole 0.

This is common for main VSERP shaped molecules like linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral.

Answer:

0.696 m

Explanation:

We'll begin by calculating the number of mole in 16.7 g of C₆H₁₂O₆. This can be obtained as follow:

Mass of C₆H₁₂O₆ = 16.7 g

Molar mass of C₆H₁₂O₆ = (6×12) + (12×1) + (6×16)

= 72 + 12 + 96

= 180 g/mol

Mole of C₆H₁₂O₆ =?

Mole = mass / molar mass

Mole of C₆H₁₂O₆ = 16.7 / 180

Mole of C₆H₁₂O₆ = 0.093 mole

Next, we shall convert 133.6 g of water to Kg. This can be obtained as follow:

1000 g = 1 Kg

Therefore,

133.6 g = 133.6 g × 1 Kg / 1000 g

133.6 g = 0.1336 Kg

Thus, 133.6 g is equivalent to 0.1336 Kg.

Finally, we shall determine the molality of the solution. This can be obtained as illustrated below:

Mole of C₆H₁₂O₆ = 0.093 mole

Mass of water = 0.1336 Kg

Molality =?

Molality = mole / mass of water (in Kg)

Molality = 0.093 / 0.1336

Molality = 0.696 m

Therefore, the molality of the solution is 0.696 m