Which of the following is an example of a Brønsted-Lowry base?
Answers
Final answer:
A Brønsted-Lowry base is a species that accepts a proton (hydrogen ion) from another species. NH3, OH-, and even water itself are examples of Brønsted-Lowry bases, denoting they accept protons.
Explanation:
A Brønsted-Lowry base is a species that can accept a proton (a hydrogen ion) from another species. For instance, in a reaction between water and ammonia, NH3 is the Brønsted-Lowry base because it accepts a proton from water. This means that any species capable of accepting a proton, such as hydroxide ion (OH-), ammonia (NH3), or water itself can be considered a Brønsted-Lowry base.
For example, think about the dissociation of water:
H2O + H2O ⇌ H3O+ + OH-
In this reaction, water is acting as both a Brønsted-Lowry acid and a Brønsted-Lowry base. One water molecule donates a proton and becomes a hydroxide ion (the conjugate base), while the other accepts a proton to become hydronium (the conjugate acid).
Another example would be the ionization of ammonia in water:
NH3 + H2O ⇌ NH4+ + OH-
Here, ammonia (NH3) is the Brønsted-Lowry base as it accepts a proton from water to become ammonium (NH4+).
Learn more about Brønsted-Lowry Base here:
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Related Questions
Reaction 2 occurs when an excess of 6 M HCI(aq) solution is added to 100. mL of NaOCl(aą) of unknown concentration. If the reaction goes to completion and 0.010 mol of Cl2(g) is produced, then what was the molarity of the NaOCl(aq) solution? (A) 0.0010 M (B) 0.010 M (C) 0.10 M (D) 1.0 M
PLEASE HELP WITH THIS ASAP
A) Balance the following equations:i) PbCl2 + AgNO3 <----> AgCl + Pb (NO3) 2ii) AlCl3 + NH4OH <----> Al(OH)3 + NH4Cliii) FeCl3 + Ca(OH)2 <----> CaCl2 + Fe(OH)3iv) Pb(ClO3)2 + K2SO4 <----> PbSO4 + KClO3v) Na + HOH <----> NaOH + H2vi) Zn + HCl <----> ZnCl2 + H2vii) Al + AgCH3COO <----> Al(CH3COO)3 + Agviii) MgO + HNO3 <----> Mg (NO3)2 + H2Oix) MnO2 <----> Mn3O4 + O2b) Why is it incorrect to alter the chemical formula when balancing an equation?
Which formula represents a polar molecule?(1) Br2 (3) CH4(2) CO2 (4) NH3
Answers
Answer:
please check image and explanation
Explanation:
First write the balance chemical reaction
CO(g)+2H2(g)⇌CH3OH(g)
To find out the equilibrium constant first need to find the concentration of each entities at equilibrium.
Rest all thing in the image
Answers
Answer:
The first step is to find the number of moles of OH⁻ that reacted with the HCl. To do this multiply 2.00L by 1.50M to get 3 moles of Ca(OH)₂. Then you multiply 3 by 2 (there are 2 moles of OH⁻ per every 1 mole of Ca(OH)₂) to get 6 moles of OH⁻. That means that you needed 6 moles of HCl since 1 mole of HCl contains 1 mole of H⁺ and equal amounts H⁺ and OH⁻ reacted with each other. To find the molarity of the HCl solution you need to divide 6mol by 1L to get 6M. Tat means that the concentration of the acid was 6M.
I hope this helps. Let me know if anything was unclear.
Explanation:
Uniform
Heterogeneous
Solutes
Homogenous
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Answer: Heterogenous
Explanation:
A heterogenous mixture is one where the composition of matter is not uniform throughout.
Some examples of heterogenous mixtures include: chocolate chip cookies, salad dressing, strawberry yogurt
A The polar substance has a lower boiling point than the nonpolar substance.
BThe nonpolar substance has a lower boiling point than the polar substance.
C Both substances have similar volatilities.
DBoth substances have similar solubilities.
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Answer:
- The correct option is B. The nonpolar substance has a lower boiling point than the polar substance.
Explanation:
- Substances with hydrogen bonding, an intermolecular force, will have much higher boiling points than those that have ordinary dipole-dipole intramolecular forces. Non-polar molecules have lower boiling points, because they are held together by the weak van der Waals forces.
Note
- However, if size of non polar increases, then its boiling point increases due to increases in van der walls forces with large size.
(2) 35.0% (4) 60.0%
Answers
Answer:
The correct option is (2) 35.0%
Explanation:
If we want to calculate the percent composition by mass of nitrogen in NH4NO3 we first need to calculate the mass of nitrogen in one mole of NH4NO3.
Because of the molecular form of NH4NO3 (it has 2 ''N'') we know that one mole of NH4NO3 contains 2 moles of N.
The molar mass of N (nitrogen) is
This means that 1 mole of N contains 14.0067 grams of N.
Because we have 2 moles of N ⇒
We know that in 1 mole of NH4NO3 we have 2 moles of N(28.0134 g of N).
To calculate the percent composition by mass of nitrogen we need to divide the mass of nitrogen in one mole of NH4NO3 by the mass of one mole of NH4NO3 and then multiply it by 100.
We know that in 1 mole of NH4NO3 there are 80.0 g of NH4NO3 (Because of the molar mass data) ⇒
% ≅ 35.0%
We find that the percent composition by mass of nitrogen in NH4NO3 is 35.0%
We conclude that the correct option is (2) 35.0%
2. hydrogen bonding
3. polar covalent bonding
4. nonpolar covalent bonding
Answers
The answer is Hydrogen bonding.
Hydrogen bonding among water molecules is responsible for the high specific heat of water the result of which water gains heat very slowly.
Specific heat is the amount of heat per unit mass that is required to raise the temperature by one degree Celsius.
The specific heat of water is 4.186 joules/gram Celcius, which is higher than any other common substance. It is higher than that of a metal.
Thus due to this, water tends to boil at high temperature.