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2 months ago

What is the molarity of potassium ions in a 0.122 M K2CrO4 solution

Chemistry

2 answers:

eduard [2.7K]2 months ago

6 0

The concentration of potassium ions in a K2CrO4 solution that is 0.122 M is 0.244 M.

Explanation

To derive the dissociation reaction for K2CrO4, we have:

K2CrO4 (aq) → 2K^+ (aq) + CrO4^2- (aq)

K2CrO4 dissociates to yield 2 potassium ions, thus the concentration of potassium ions = 2 x 0.122 = 0.244 M.

eduard [2.7K]2 months ago

4 0

Answer: The concentration of potassium ions in a $K_2CrO_4$ solution is 0.244 M

Explanation:

The dissociation reaction of $K_2CrO_4$ in solution is as follows:

$K_2CrO_4\rightarrow 2K^++CrO_4^{2-}$

From this reaction, we find that one mole of $K_2CrO_4$ dissociates in solution to form 2 moles of $K^+$ (potassium ion) and 1 mole of $CrO_4^{2-}$ (chromate ion).

According to the question,

0.122 M of $K_2CrO_4$ dissociates in solution resulting in $2\times 0.122M=0.244M$ of $K^+$ (potassium ion) and 0.122 M of $CrO_4^{2-}$ (chromate ion).

Therefore, the concentration of potassium ions in a $K_2CrO_4$ solution is 0.244 M

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A 85.2 g copper bar was heated to 221.32 degrees Celsius and placed in a coffee cup calorimeter containing 4250 mL of water at 2

eduard [2782]

Answer:- 64015 J

Solution: The calorimeter contains 4250 mL of water, which is at a temperature of 22.55 degrees Celsius.

The water's density is 1 gram per mL.

Thus, the mass of water = $4250mL(\frac{1g}{1mL})$ = 4250 grams.

After introducing the hot copper bar, the final temperature of the water reaches 26.15 degrees Celsius.

Thus, $\Delta T$ for the water = 26.15 - 22.55 = 3.60 degrees Celsius.

The specific heat capacity of water is 4.184 $\frac{J}{g.^0C}$ .

To determine the heat absorbed by the water, we can use the following formula:

$q=mc\Delta T$

where q represents heat energy, m refers to mass, and c indicates specific heat.

Now let's substitute the values into the equation to perform the calculations:

$q=4250g*\frac{4.184J}{g.^0C}*3.60^0C$

q = 64015 J

Therefore, the water absorbs 64015 J of heat.

5 0

2 months ago

How many moles of O are in 2.45 moles of H2CO3?

alisha [2963]

7.35 moles of oxygen. Initially, for each mole of H₂CO₃, there are 3 moles of oxygen, as derived from the acid's formula. For 2.45 moles of the compound stated in the problem, which is carbonic acid, we calculate: If 1 mole of H₂CO₃ corresponds to 3 moles of oxygen, then for 2.45 moles of H₂CO₃, we have X moles of oxygen. Thus, X = (3 × 2.45) / 1 = 7.35 moles of oxygen.

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1 month ago

Combustion analysis of a 13.42-g sample of the unknown organic compound (which contains only carbon, hydrogen, and oxygen) produ

lions [2927]

Answer: The molecular formula for the specified organic compound is $C_{18}H_{20}O_2$

Explanation:

The combustion reaction of a hydrocarbon comprising carbon, hydrogen, and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where 'x', 'y', and 'z' denote the subscripts of Carbon, hydrogen, and oxygen respectively.

The information provided includes:

Mass of $CO_2=39.61g$

Mass of $H_2O=9.01g$

From our knowledge:

Molar mass of carbon dioxide is 44 g/mol

Molar mass of water is 18 g/mol

For determining the amount of carbon:

In carbon dioxide weighing 44 g, 12 g of carbon is found.

Hence, in 39.61 g of carbon dioxide, $\frac{12}{44}\times 39.61=10.80g$ grams of carbon will be found.

For finding the mass of hydrogen:

In water weighing 18 g, 2 g of hydrogen can be found.

Thus, in 9.01 g of water, $\frac{2}{18}\times 9.01=1.00g$ grams of hydrogen will be present.

Mass of oxygen in the compound is given by (13.42) - (10.80 + 1.00) = 1.62 g

To derive the empirical formula, the following steps must be followed:

Step 1: Convert the indicated masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{10.80g}{12g/mole}=0.9moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1g}{1g/mole}=1moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{1.62g}{16g/mole}=0.10moles$

Step 2: Calculating the ratio of moles of the respective elements.

To find the mole ratio, each mole value is divided by the smallest amount of moles calculated, which is 0.10 moles.

For Carbon = $\frac{0.9}{0.10}=9$

For Hydrogen = $\frac{1}{0.10}=10$

For Oxygen = $\frac{0.10}{0.10}=1$

Step 3:Using the mole ratios as subscripts.

The ratio of C: H: O = 9: 10: 1

Therefore, the empirical formula for the mentioned compound is $C_9H_{10}O$

To ascertain the molecular formula, it is necessary to find the valency, which is multiplied by each element to derive the molecular formula.

The equation to determine the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

Given the data:

Molecular formula mass = 268.34 g/mol

Empirical formula mass = 134 g/mol

Substituting the values into the aforementioned equation yields:

$n=\frac{268.34g/mol}{134g/mol}=2$

By multiplying this valency with each element's subscripts from the empirical formula, the results are:

$C_{(9\times 2)}H_{(10\times 2)}O_{(1\times 2)}=C_{18}H_{20}O_2$

Consequently, the molecular formula for the given organic compound is $C_{18}H_{20}O_2$ .

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1 month ago

Several amino acids are intermediates of the urea cycle, having side ammonia groups that join with free carbon dioxide (CO2) and

Alekssandra [3086]

Response:

A. Arginine

Clarification:

The urea cycle consists of biochemical processes that convert ammonia into urea.

Steps of the urea cycle:

Carbamoyl phosphate reacts with ornithine transcarbamoylase to form citrulline through the release of a phosphate group along with ornithine.
In the presence of argininosuccinate synthetase, the amino group from aspartate and the carbonyl from citrulline combine to create argininosuccinate. This reaction requires ATP.
Subsequently, argininosuccinate is split by argininosuccinase to yield arginine and fumarate.
Then, arginine is broken down by arginase to produce urea and ornithine. Ornithine is recycled back to mitochondria, restarting the urea cycle.

7 0

2 months ago

Write the formulas for the following ionic compounds: (a) copper bromide (containing the Cu+ ion), (b) manganese oxide (containi

Anarel [2989]

Answer: The formulas for the ionic compounds are:

a) $CuBr$

b) $Mn_2O_3$

c) $Hg_2I_2$

d) $Mg_3(PO_4)_2$

Explanation:

Determining the formulas for ionic compounds relies on:

The criss-cross method, wherein the oxidation states of ions are exchanged, forming the subscripts of the respective ions, resulting in a neutral compound.

(a) Copper bromide is formed based on the $Cu^+$ ion.