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2 years ago

For each group of compounds listed, which is the strongest acid? I. HIO2, HIO3, HIO4 II. H2Se, H2S, H3As III. HPO2, HClO2, HBrO2

Chemistry

1 answer:

DIA [1.3K]2 years ago

7 0

Answer:

In group I, strongest acid is $HIO_4$

In group II, the strongest acid is $H_2Se$

In group III, the strongest acid is $HClO_2$

Explanation:

Group I:

Acidic strength depends upon the stability of conjugated base formed after release of H+.

In the given acids, after releases of H+ following conjugate bases are formed:

$HIO_2 \rightarrow H^+ + IO_2^-\\HIO_3 \rightarrow H^+ + IO_3^-\\HIO_4 \rightarrow H^+ + IO_4^-$

In $IO_4^-$ , negative charge is distributed over three electronegative atom 'O' which makes it more stable as compared to other two conjugate bases.

Therefore, $HIO_4$ is trongest acid among given.

Group II:

H-Se bond is weaker than H-S bonds which makes it more acidic as breaking of H-Se bond is easier to release H+.

In case of $H_3As$ , As is less electronegative than Se. Because of more electronegative nature of Se, electrons of H-Se bond are attracted towards Se and so removal of H+ is easier.

So $H_2Se$ is the strongest acid among give.

Group III:

Acidity is also affected by bond distance and electronegativity of the central element.

Here, electronegativity dominates over bond distance.

Cl has the highest electronegativity among given. Because of hugh electronegativity, electrons are attracted towards Cl, and release of H+ becomes easier as compared to other two.

So, $HClO_2$ is the strongest acid among given.

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How many iodide ions are present in 65.5ml of .210 m AlI3 solution

blondinia [14]

Answer:

$2.48\times 10^{22} ions$ are present in solution.

Explanation:

Molarity of the solution = 0.210 M

Volume of the solution = 65.5 ml = 0.0655 L

Moles of aluminum iodide= n

$Molarity=\frac{\text{Moles of compound}}{\text{Volume of the solution(L)}}$

$0.210M=\frac{n}{0.0655 L}$

n = 0.013755 moles of aluminum iodide

1 mole of aluminum iodide contains 3 moles of iodide ions:

Then 0.013755 moles of aluminum iodide will contain:

$3\times 0.013755 moles=0.041265 mol$ of iodide ions

Number of iodide ions in 0.041265 moles:

$0.041265 mol\times 6.022\times 10^{23}=2.48\times 10^{22} ions$

$2.48\times 10^{22} ions$ are present in solution.

7 0

2 years ago

If you compared 1 m solutions, was a 1 m nacl solution more or less hypertonic than a 1 m sucrose solution? what is your evidenc

igor_vitrenko [27]

When you say the solution is hypertonic, it means that the solution has a higher osmotic pressure. The formula for this is:

P = iMRT,
for strong electrolytes, i = number of ions.
for nonelectrolytes, i = 1

1. The P for sucrose solution which is a nonelectrolyte (assuming room temp):
P = (1)(1m)(8.314 J/mol-K)(298 K)
P = 2477.572 Pa

The P for NaCl solution, which is a strong electrolyte:
P = (2)(1 m)(8.314)(298 K)
P = 4955.144 Pa

So, that means that NaCl is more hypertonic than the sucrose solution.

2. For the second question, the P for the combination of 1 m glucose (nonelectrolyte) and 1 m sucrose is:
P = (1)(1 m)(8.314)(298 K) + (1)(1)(8.314)(298 K) = 4955.144 Pa
In this case, the osmotic pressures are now equal. It is not hypertonic, but isotonic.

7 0

2 years ago

Quinine, an antimalarial drug, is 8.63% nitrogen. There are two nitrogen atoms per molecule. What is the molecular weight of qui

Furkat [3]

Answer:

324.18 g/mol

Explanation:

Let the molecular mass of the antimalarial drug, Quinine is x g/mol

According to question,

Nitrogen present in the drug is 8.63% of x

So, mass of nitrogen = $\frac {8.63}{100}\times x$

Also, according to the question,

2 atoms are present in 1 molecule of the drug.

Mass of nitrogen = 14.01 amu = 14.01 g/mol (grams for 1 mole)

So, mass of nitrogen = 14.01×2 = 28.02

These 2 must be equal so,

$\frac {8.63}{100}\times x=28.02$

solving for x, we get:

x = 324.18 g/mol

6 0

2 years ago

If you have 10.0 grams of citric acid with enough baking soda (nahco3 how many moles of carbon dioxide can you produce?

kap26 [50]

Easy stoichiometry conversion :)

So, for stoichiometry, we always start with our "given". In this case, it would be the 10.0 grams of NaHCO3. This unit always goes over 1.

So, our first step would look like this:

10.0
------
1

Next, we need to cancel out grams to get to moles. To do this, we will do grams of citric acid on the BOTTOM of the next step, so it cancels out. This unit in grams will be the mass of NaHCO3, which is 84.007. Then, we will do our unit of moles on top. Since this is unknown, it will be 1.

So, our 2nd step would look like this:

1 mole CO2
-----------------
84.007g NaHCO3

When we put it together: our complete stoichiometry problem would look like this:

10.0g NaHCO3 1mol CO2
---------------------- x -------------------------
1 84.007g NaHCO3

Now to find our answer, all we need to do is:
Multiply the two top numbers together (which is 10.0)
Multiply the two bottom numbers together (Which is 84.007)

And then....

Divide the top answer by the bottom answer.

10.0/84.007 is 0.119

So, from 10.0 grams of citric acid, we have 0.119 moles of CO2.

Hope I could help!

6 0

2 years ago

Read 2 more answers

The easiest way to determine whether a process is exothermic or endothermic is to note the change in temperature in a calorimete

Kryger [21]

Answer:

In the calorimeter, water is the exothermic. The salt LiCI, which will dissolve, is the endothermic. The final temperature of the water after the dissolution of LiCI was lower than the initial temperature, meaning the process is exothermic. In the microscopic view of the disspolution of LiCI, water molecules were seen to move slowly as they gained energy.

Explanation:

Exothermic is a process in which heat is released during the process. Endothermic reactions absorbs heat from surrounding during a chemical process. The dissolution of salt into water is an exothermic reaction. During this process heat is release and water molecules are broken down which are surrounded by salt ions.

5 0

2 years ago