Answer:
The solution 0.010 M has a higher percent ionization of the acid.
Explanation:
The percent ionization can be found using the following equation:
[tex]\% I = \frac{[H_{3}O^{+}]}{[CH_{3}COOH]} \times 100[/tex]
Since we know the acid concentration in the two cases, we need to find [H₃O⁺].
By using the dissociation of acetic acid in the water we can calculate the concentration of H₃O⁺ in the two cases:
1. Case 1 (0.1 M):
CH₃COOH(aq) + H₂O(l) ⇄ CH₃COO⁻(aq) + H₃O⁺(aq) (1)
0.1 - x x x
[tex] Ka = \frac{[CH_{3}COO^{-}][H_{3}O^{+}]}{[CH_{3}COOH]} [/tex] (2)
Where:
Ka: is the dissociation constant of acetic acid = 1.7x10⁻⁵.
[tex] 1.7 \cdot 10^{-5} = \frac{x^{2}}{0.1 - x} [/tex]
[tex] 1.7 \cdot 10^{-5}*(0.1 - x) - x^{2} = 0 [/tex]
By solving the above equation for x we have:
x = 1.29x10⁻³ M = [CH₃COO⁻] = [H₃O⁺]
Hence, the percent ionization is:
[tex] \% I = \frac{1.29 \cdot 10^{-3} M}{0.1 M} \times 100 = 1.29 \% [/tex]
2. Case 2 (0.01 M):
The dissociation constant from reaction (1) is:
[tex] Ka = \frac{[CH_{3}COO^{-}][H_{3}O^{+}]}{[CH_{3}COOH]} [/tex]
With [CH₃COOH] = 0.01 M
[tex] 1.7 \cdot 10^{-5} = \frac{x^{2}}{0.01 - x} [/tex]
[tex]1.7 \cdot 10^{-5}*(0.01 - x) - x^{2} = 0[/tex]
By solving the above equation for x:
x = 4.04x10⁻⁴ M = [CH₃COO⁻] = [H₃O⁺]
Then, the percent ionization for this case is:
[tex] \% I = \frac{4.04 \cdot 10^{-4} M}{0.01 M} \times 100 = 4.04 \% [/tex]
As we can see, the solution 0.010 M has a higher percent ionization of the acetic acid.
Therefore, the solution 0.010 M has a higher percent ionization of the acid.
I hope it helps you!
The 0.010 M solution of CH₃COOH has a higher percent ionization compared to the 0.10 M solution.
Percentage ionization formulaThe percent ionization of the acid solution is determined using the following equation:
Percent ionization = [H₃O⁺]/[CH₃COOH]What is the ionization equation of CH₃COOHIonization equation of CH₃COOH is given below:
CH₃COOH + H₂O ⇄ CH₃COO⁻ + H₃O⁺
Ka = 1.7 * 10⁻⁵
Ka = [CH₃COO⁻][H₃O⁺]/[CH₃COOH]Calculating [H₃O⁺]The [H₃O⁺] in both solutions is determined first.
For the 0.1 M solution:
CH₃COOH(aq) + H₂O(l) ⇄ CH₃COO⁻(aq) + H₃O⁺(aq) (1)
0.1 - x x x
Using the equation of dissociation constant:
Ka = [CH₃COO⁻][H₃O⁺]/[CH₃COOH]
1.7 * 10⁻⁵ = x₂/0.1 - x
assuming x is very small;
x = 1.29 * 10 ⁻³ M
Hence, [H₃O⁺] = 1.29 * 10 ⁻³ M
For the 0.010 M solution
CH₃COOH(aq) + H₂O(l) ⇄ CH₃COO⁻(aq) + H₃O⁺(aq) (1)
0.01 - x x x
Using the equation of dissociation constant:
Ka = [CH₃COO⁻][H₃O⁺]/[CH₃COOH]
1.7 * 10⁻⁵ = x₂/0.01 - x
assuming x is very small;
x = 4.04 * 10 ⁻⁴ M
Hence, [H₃O⁺] = 4.04 * 10 ⁻⁴ M
Calculating the percent ionizationFor the 0.1 M solution
Percent ionization = (1.29 * 10 ⁻³ M/0.1) * 100%
Percent ionization = 1.29%
For the 0.01 M solution:
Percent ionization = (4.04 * 10 ⁻⁴ M/0.1) * 100%
Percent ionization = 4.04 %
Therefore, the 0.010 M solution of CH₃COOH has a higher percent ionization compared to the 0.10 M solution.
Learn more about percent ionization at: https://brainly.com/question/15073874
What can the flow of electrons be easily compared to?
a.The flow of mud
b.The flow of water
c.The flow of wind
d.The flow of gravity
can you make energy with ionized particles? yes or no and how
mass
6.00 g of a certain compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 180. g/mol, is burned
completely in excess oxygen, and the mass of the products carefully measured:
product
carbon dioxide 8.80 g
3.60 g
Use this information to find the molecular formula of X.
water
alo
O
х
?
The molecular formula =C₆H₁₂O₆
Further explanationGiven
6.00 g of a certain compound X
The molecular molar mass of 180. g/mol
CO₂=8.8 g
H₂O=3.6 g
Required
The molecular formula
Solution
mass C in CO₂ :
= 1.12/44 x 8.8
= 2.4 g
mass H in H₂O :
= 2.1/18 x 3.6
= 0.4 g
Mass O in compound :
= 6-(2.4+0.4)
= 3.2 g
Mol ratio C : H : O
= 2.4/12 : 0.4/1 : 3.2/16
= 0.2 : 0.4 : 0.2
= 1 : 2 : 1
The empirical formula : CH₂O
(CH₂O)n=180 g/mol
(12+2+16)n=180
(30)n=180
n=6
(CH₂O)₆=C₆H₁₂O₆
What is meant by the term average mass
Answer:
Explanation:
The average atomic mass (sometimes called atomic weight) of an element is the weighted average mass of the atoms in a naturally occurring sample of the element. Average masses are generally expressed in unified atomic mass units (u), where 1 u is equal to exactly one-twelfth the mass of a neutral atom of carbon-12.
A homogeneous mixture is?
Answer:
two components of the same thing
Explanation:
How many moles are in 60.0 grams of water?
3.33 mol H₂O
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableUsing Dimensional AnalysisExplanation:Step 1: Define
60.0 g H₂O (Water)
Step 2: Identify Conversions
Molar Mass of H - 1.01 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of H₂O - 2(1.01) + 16.00 = 18.02 g/mol
Step 3: Convert
Set up: [tex]\displaystyle 60.0 \ g \ H_2O(\frac{1 \ mol \ H_2O}{18.02 \ g \ H_2O})[/tex]Multiply: [tex]\displaystyle 3.32963 \ mol \ H_2O[/tex]Step 4: Convert
Follow sig fig rules and round. We are given 3 sig figs.
3.32963 mol H₂O ≈ 3.33 mol H₂O
HURRY HELP 10 POINTS ILL GOVE BRAINLIEST I HAVE TO PASS PICTURE PROVIDED
Answer:
C₃H₄O₄
Explanation:
In order to get the empirical formula of a compound, we have to follow a series of steps.
Step 1: Divide the percent by mass of each element by its atomic mass.
C: 34.6/12.01 = 2.88
H: 3.9/1.01 = 3.86
O: 61.5/16.00 = 3.84
Step 2: Divide all the numbers by the smallest one, i.e., 2.88
C: 2.88/2.88 = 1
H: 3.86/2.88 ≈ 1.34
O: 3.84/2.88 ≈ 1.33
Step 3: Multiply all the numbers by a number that makes all of them integer
C: 1 × 3 = 3
H: 1.34 × 3 = 4
O: 1.33 × 3 = 4
The empirical formula is C₃H₄O₄.
Suppose a current of 220.mA is passed through an electroplating cell with an aqueous solution of AgNO3 in the cathode compartment for 79.0 seconds. Calculate the mass of pure silver deposited on a metal object made into the cathode of the cell.
Answer:
0.0195 g
Explanation:
Ag^+(aq) + e -------> Ag(s)
Since 1 electron was transferred, that means 96500C of electricity was required
108 g is deposited 96500 C
xg is deposited 220 × 10^-3 × 79.0
x = 108 × 220 × 10^-3 × 79.0/96500
x= 19.5 × 10^-3 g
x= 0.0195 g
What is the molar mass of CuCIO3
147.05 g/mol
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableExplanation:Step 1: Define
CuClO₃
Step 2: Find MM
Molar Mass of Cu - 63.55 g/mol
Molar Mass of Cl - 35.45 g/mol
Molar Mass of O - 16.00 g/mol
Molar Mass of CuClO₃ - 63.55 + 35.45 + 3(16.00) = 147.05 g/mol
17. Which of the following
hydrocarbon undergo addition
reaction:
С3Н6
С2Н6
ОООО
С3Н8
CH4
Answer:
С3Н6.
Explanation:
Hello!
In this case, since addition reactions imply that a radical or some radicals are added to the parent chain, we notice that only unsaturated hydrocarbons are able to undergo addition whereas saturated ones undergo substitution reactions as they already have all the carbon bonds bonded to leaving groups.
In such a way, we can rule out C2H6, C3H8 and CH4 as they are all alkanes; therefore, only С3Н6 is able to undergo an addition reaction due to the C=C which is able to lose one of those bonds and allow an incoming radical to get included into the parent chain.
Best regards!
What is the mass in grams of 2.25 mol of the element iron, Fe?
126 g Fe
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableUsing Dimensional AnalysisExplanation:Step 1: Define
2.25 mol Fe
Step 2: Identify Conversions
Molar Mass of Fe - 55.85 g/mol
Step 3: Convert
Set up: [tex]\displaystyle 2.25 \ mol \ Fe(\frac{55.85 \ g \ Fe}{1 \ mol \ Fe})[/tex]Multiply: [tex]\displaystyle 125.663 \ g \ Fe[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
125.663 g Fe ≈ 126 g Fe
How many moles of calcium, Ca, are in 5.00 g of calcium?
0.125 mol Ca
General Formulas and Concepts:Math
Pre-Algebra
Order of Operations: BPEMDAS
Brackets Parenthesis Exponents Multiplication Division Addition Subtraction Left to RightChemistry
Atomic Structure
Reading a Periodic TableUsing Dimensional AnalysisExplanation:Step 1: Define
5.00 g Ca
Step 2: Identify Conversions
Molar mass of Ca - 40.08 g/mol
Step 3: Convert
Set up: [tex]\displaystyle 5.00 \ g \ Ca(\frac{1 \ mol \ Ca}{40.08 \ g \ Ca})[/tex]Multiply: [tex]\displaystyle 0.12475 \ mol \ Ca[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
0.12475 mol Ca ≈ 0.125 mol Ca
Two electron(s) are removed from an carbon atom. Enter the chemical symbol of the element.
Answer:
[tex]C^{2+}[/tex]
Explanation:
When a proton is removed, it changes the whole element. However, when electrons are removed, it becomes an ion. Since we are removing two electrons, we are subtracting a negative number, giving us positive two as our net ionic charge. Therefore, the answer is [tex]C^{2+}[/tex]
A sample of 25.0 mL of 0.120 M Ca(OH)2(aq) is titrated with 0.150 M HCl(aq). What volume of HCl(aq) is needed to completely neutralize the Ca(OH)2(aq)
Answer:
[tex]V_{HCl}=48.0 mL[/tex]
Explanation:
Hello!
In this case, since the reaction between calcium hydroxide and hydrochloric acid shows a 2:1 mole ratio between them:
[tex]2HCl+Ca(OH)_2\rightarrow CaCl_2+2H_2O[/tex]
We need to use the following mole ratio:
[tex]2n_{Ca(OH)_2}=n_{HCl}[/tex]
That can be written in volumes and concentrations:
[tex]2M_{Ca(OH)_2}V_{Ca(OH)_2}=M_{HCl}V_{HCl}[/tex]
Thus, we solve for the volume of HCl as it is the unknown:
[tex]V_{HCl}=\frac{2M_{Ca(OH)_2}V_{Ca(OH)_2}}{M_{HCl}}[/tex]
Therefore, we plug in to obtain:
[tex]V_{HCl}=\frac{2*0.120M*25.0mL}{0.150M} \\\\V_{HCl}=48.0 mL[/tex]
Best regards!
Salad oil floats on water. Water has a density of 1.0 g/cm3. What can you say about the density of the salad oil?
Answer:
Density of the oil is lesser than that of the water
Explanation:
The density of water is given as 1.0g/cm³.
Salad oil is found to float on water, this implies that the density of this salad oil is lesser than that of the water.
When the density of a substance is greater than another, it will sink. If the density of the salad oil is greater than that of water, then it will sink and not float. Since the oil floats on water, the density of the oil is lesser than that of the water.Density is the mass per unit volume of a substance.
butyric acid has a putrid odor like rancid butter. If you got some of this material on your hands, how could you remove the odor
Answer:
The correct answer would be - the easiest way is to wash with some polar solvent or salt solution or soap and water
Explanation:
Butyric acid is a carboxylic acid that has a putrid odor like rancid butter. If an individual touch this chemical will have the same odor on his hand and to get rid of it one should wash his hand with a polar solvent such as methanol, or salt solutions such as like NaHCO3, or soap and water that will form sodium butyrate that has no smell and easily dissolve and remove.
Thus, the easiest way is to wash with some polar solvent or salt solution or soap and water
Calculate the percentage of water in the compound CaSO4 x 6H2O
The percentage of water in the compound CaSO₄.6H₂O = 44.26%
Further explanationGiven
Compound CaSO₄. 6H₂O
Required
The percentage of water
Solution
MW CaSO₄. 6H₂O :
= 40 + 32 + 4.16 + 12.1 + 6.16
= 244
MW 6H2O :
= 12.1 + 6.16
= 108
%water = (108 : 244) x 100%
%water = 44.26
The percentage of water in the compound CaSO₄.6H₂O is 44.26%
Calculation of percentage:Since MW CaSO₄. 6H₂O :
= 40 + 32 + 4.16 + 12.1 + 6.16
= 244
Now
MW 6H2O :
= 12.1 + 6.16
= 108
So, percentage of water = (108 : 244) x 100%
= 44.26
learn more about water here: https://brainly.com/question/5534000
To what temperature must an ideal gas at 27 o C be cooled to reduce its volume by 1/3
Answer:
28 oc
Explanation:
Of the following, which most likely involves a chemical reaction?
NEED ASAP PLEASE
Select one:
a. Boiling water turns a fresh egg into a hard boiled egg.
b. Dissolving salt in water produces a transparent liquid.
c. A huge wave knocks down a beach home.
d. Wind turns a generator to produce electricity.
a ______ is a single kind of matter that has a specific composition.
Answer:
SUBSTANCE
Explanation:
hope that help you thanx
What is the mass, in grams, of 0.0490 mol of iron(III) phosphate
Answer:
m = 7.39 g.
Explanation:
Hello!
In this case, since the molar mass of iron (III) phosphate is 150.82 g/mol based on its molecular formula (FePO₄), we can compute the mass in grams of 0.0490 moles of this compound by setting up the following dimensional analysis:
[tex]m=0.0490mol*\frac{150.82g}{1mol} \\\\m=7.39 g[/tex]
Best regards!
Write out an example of a single replacement reaction involving silver and zinc.
Answer:
whats zinc?
Explanation:
Which characteristic is used to classify metamorphic rocks as foliated or non-foliated?
Answer: d. Arrangement of grains
Explanation:
Edge:)))
The frequency of the stretching vibration of a bond in IR spectroscopy depends on what two quantities?
Answer:
Strength of the bond
Masses of the bonded atoms.
Explanation:
The lack of such groups means that they are not endogenous in the concentrate. 1. A bond's spreading frequency relies on the frequency of the bond and the concentrations of the atoms that are bonded.
When does a chemical bond form between two atoms? Select one :
O a. When attractive forces are greater than repulsive forces.
O b. When potential energy is lowest for the pair.
O c. When potential energy is greatest for the pair .
O d. When repulsive forces are greater than attractive forces.
Complete combustion of 3.10 g of a hydrocarbon produced 9.90 g of CO2 and 3.55 g of H2O. What is the empirical formula for the hydrocarbon
Answer: C9H16
Explanation:
molar mass C = 12.011, H = 1.008, O = 15.999, CO2 = 44.01, H2O = 18.00
9.9g CO2 = 0.225 mol, 3.55 g H2O = 0.200 mol
long way
molecules CO2 = 1.355x10^23 —> atoms of C
molecules H2O = 1.204x10^23 —> molecules H2
C:H2 = 1.355/1.204 = 1.125. —> C9H16
short way
molar massesCO2:H2O = 0.225:0.2 = 9:8
–> C9H16
verify
molar mass C9H16 =124
3.1g = 0.025 mol
oxidise C9H16 + 13O2 —> 9CO2 + 8H2O
0.025 mol + 13*0.025 mol (0.35mol) —> 9*0.025 + 8*0.025 —> 0.0.225 + 0.2
A student adds 34.2 mL of water to 72.3 mL of a 7.50 M glucose solution. (i) Will this solution be concentrated or dilute
Answer:
The solution will be dilute
Explanation:
The concentration of a solution is defined as the ratio between an amount of solute (Glucose, in this case) and an amount of solvent (Water in this case).
As the student is adding some water (Solvent), the amount of solute per amount of solvent will decrease. That is, if the concentration decreases,
the solution will be dilute
HELP ME SLOVE RN IT IS FOR CHEM
Answer:
NARUTOOOO
Explanation:
CONVERSIONS
Complete the following conversions
3. Given the following reaction, how many moles of Al2O3 will be produced if 1.35 moles of Fe are produced?
(8 points)
2 AI 3 Feo
3 Fe + Al2O3
+
it’s number 3 pls help
Answer:
Number of moles of Al₂O₃ = 0.45 mol
Explanation:
Given data:
Number of moles of Fe produced = 1.35 mol
Number of moles of Al₂O₃ = ?
Solution:
2Al + 3FeO → 3Fe + Al₂O₃
now we will compare the moles of iron and Al₂O₃
Fe : Al₂O₃
3 : 1
1.35 : 1/3×1.35 = 0.45 mol
the system that acts as a barrier from the outside the environment is called________
The air barrier system