It is common for students to overshoot the endpoint, meaning they add too much NaOH(aq) from the buret, which causes the solution to turn bright pink. What specific impact does this mistake have on the percent of acetic acid result?
Answers
Answer: the percentage of acetic acid will be low.
Explanation: The major aim during titration of acids and bases is to determine the endpoint , that is exact point where the acid in the beaker changes colour, (in this case, pink )with an additional drop from the burette containing the base, since it is usually difficult to mark the equivalence point that tells us when all the substrate in the beaker has been neutralized completely with the buretted substance.
Overshooting the end point is an error which can occur when the person involved in the the titration accidently goes beyond this endpoint by adding too much of the substance(base) from the burette into the beaker missing the exact endpoint.
This implies that the person has added too much of the burreted liquid, ie the base than required , making the acid in the beaker to continue to react resulting to a lower concentration of the acid (acetic acid) with excess base.(NaOH)
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Answers
Answer:
Magnesium hydroxide, Mg(OH)2, is an Arrhenius base and therefore also a Brønsted-Lowry base.
However, water can also act as a base by accepting a proton from an acid to become its conjugate base, H3O+. where Al(OH)3 is acting as a Lewis Base.
Explanation:
Arrhenius acids and bases
An Arrhenius acid is any species that increases the concentration of H+start text, H, end text, start superscript, plus, end superscript in aqueous solution.
An Arrhenius base is any species that increases the concentration of OH−start text, O, H, end text, start superscript, minus, end superscript in aqueous solution.
Answers
- C=C : 835
- C≡C : 612
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Answer:
The order of increasing bond lenght :
-C≡C < -C=C < -C-C
Explanation:
Bond length is defined as average distance between two nuclei of bonded atoms in a molecule.Bond length is inversely proportional to the number of bonds present between two atoms.
...[1]
Bond energy is defied as amount of energy required to break apart the bond of 1 mole of molecule into their individual atom.
Bond energy is directly proportional to the number of bonds present between two atoms.
..[2]
From [1] and [2]:
Bond : Energy (kJ/mol)
-C-C : 346
-C=C : 612
-C≡C : 835
The order of decreasing bond energy :
835 kJ/mol > 612 kJ/mol > 346 kJ/mol
The order of increasing bond lenght :
-C≡C < -C=C < -C-C
Answers
Considering the definition of molar mass, 1.26 moles are in 98.3 grams of aluminum hydroxide, Al(OH)₃.
The given molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
The molar mass of a compound (also called Mass or Molecular Weight) is the sum of the molar mass of the elements that form it (whose value is found in the periodic table) multiplied by the number of times they appear in the compound.
In this case, you know the molar mass of the elements is:
- Al= 27 g/mole
- O= 16 g/mole
- H= 1 g/mole
So, the molar mass of the compound Al(OH)₃ is calculated as:
Al(OH)₃= 27 g/mole + 3× (16 g/mole + 1 g/mole)
Solving:
Al(OH)₃= 78 g/mole
Next, you can apply the following rule of three: if 78 grams of the compound are contained in 1 mole, 98.3 grams are contained in how many moles?
amount of moles= 1.26 moles
1.26 moles are in 98.3 grams of aluminum hydroxide, Al(OH)₃.
Learn more:
Atomic mass (Al)=27 amu
Atomic mass (O)=16 amu
Atomic mass (H)=1 amu
molecular weight= 27 amu+3(16 amu + 1 amu) =78 amu.
Therefore, the molar mass of Al (OH)₃ is 78 g/ mol
Now, we calculate the number of moles in 98.3 g of aluminum hydroxide.
78 g-------------------1 mol
98.3 g----------------- x
x=(98.3 g * 1 mol) / 78 g=1.26 moles.
Answer: 1.26 moles.
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The answer is True, I've taken this test.
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Answer: Here are the steps to determine the atomic mass of an element with isotopic forms:
1. Identify the isotopes: Determine the different isotopic forms of the element. Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons.
2. Determine the relative abundance: Find the relative abundance of each isotope. This information is typically given as a percentage or decimal. The relative abundance represents the proportion or percentage of each isotope in a naturally occurring sample of the element.
3. Obtain the mass of each isotope: Identify the mass of each isotope. This is usually given in atomic mass units (u) or grams per mole (g/mol).
4. Multiply the mass of each isotope by its relative abundance: Multiply the mass of each isotope by its relative abundance (expressed as a decimal). This calculates the contribution of each isotope to the overall atomic mass.
5. Sum the contributions: Add up the contributions of each isotope to obtain the atomic mass. This sum represents the weighted average of the masses of all the isotopic forms, taking into account their relative abundance.