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3 years ago

Which of the following are produced when a base is dissolved in water?

Chemistry

2 answers:

Sergeeva-Olga [200]3 years ago

6 0

$\boxed{{\text{B}}{\text{. Hydroxide ions}}}$ are produced when a base is dissolved in water.

Further explanation:

Definitions of acids and bases according to different theories:

1. Arrhenius theory

This theory defines acid as the one that produces hydrogen or hydronium ions in the solution, while the base is the one that produces hydroxide ions in the solution. HBr, ${\text{HN}}{{\text{O}}_3}$ and ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$ are examples of Arrhenius acids whereas NaOH and KOH are Arrhenius bases.

2. Bronsted-Lowry theory

It describes acid as the species that donates a proton in the reaction while base accepts a proton. ${{\text{H}}_2}{\text{O}}$ is a Bronsted acid and ${\text{N}}{{\text{H}}_3}$ is a Bronsted base.

3. Lewis theory

According to this theory, an acid accepts a pair of electrons to electron-rich species and a base donates electrons to electron-deficient species in the reaction. ${\text{B}}{{\text{F}}_3}$ and ${\text{S}}{{\text{O}}_3}$ are Lewis acids while ${{\text{H}}_2}{\text{O}}$ and ROH are the examples of Lewis base.

According to the Arrhenius definition, the base is the one that produces hydroxide ions when dissolved in water. For example, NaOH is a base. The dissociation reaction of NaOH in water is as follows:

${\text{NaOH}} + {{\text{H}}_{\text{2}}}{\text{O}} \to {\text{N}}{{\text{a}}^ + } + {\text{O}}{{\text{H}}^ - }$

Therefore option B is correct.

Learn more:

The reason for the acidity of water brainly.com/question/1550328
Reason for the acidic and basic nature of amino acid. brainly.com/question/5050077

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Acid, base and salts

Keywords: acid, base, electrons, protons, Arrhenius theory, Lewis theory, Bronsted-Lowry theory, hydrogen, hydronium ion, hydroxide ion, accept, donate, NaOH, HCl, ROH, H2O, Na+, OH-, H+, BF3, SO3, NH3, KOH, H2SO4.

Irina-Kira [14]3 years ago

3 0

Answer is: B. Hydroxide ions.

An Arrhenius base is a substance that dissociates in water to form hydroxide ions (OH⁻).

For example sodium hydroxide: NaOH(aq) → Na⁺(aq) + OH⁻(aq).

Another example, balanced chemical reaction: Ba(OH)₂(aq) → Ba²⁺(aq) + 2OH⁻(aq).

According to the Arrhenius definition barium hydroxide is base.

Acids and bases when react (neutralisation) produce salt and water.

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When a piece of zinc metal is carefully placed in a beaker of strong acid, bubbles form on the surface of the metal and begin to

kati45 [8]

Answer:

A. a new substance is being produced.

Explanation:

The bubbles most likely indicates that a new substance is being produced by this reaction. In essence, we describe this sort of change as chemical change.

In a chemical change, new substances are usually produced. They are accompanied by the evolution or absorption of energy.

The reaction of Zinc with a strong acid to produce bubbles on the surface of the metal indicates a chemical change and the formation of a new kind of substance.

Take for example, let zinc reacts with hydrocholoric acid, HCl;

Zn + 2HCl → ZnCl₂ + H₂

Since Zn is higher than Hydrogen in the activity series, it will displace it from HCl and liberate hydrogen gas as a product. This will cause the bubbles observed in the reaction.

This is a chemical change and new products have been formed.

B and D are wrong because they are both physical changes.

C is wrong because no information about such is provided by the problem statement.

So, when a piece of zinc metal combines with a strong acid, a new kind of substance is produced.

8 0

3 years ago

Which of the following is altered by a catalyst?

Vika [28.1K]

In chemistry, a catalyst can speed up the reaction (or make it initiate easier) by altering the activation energy, lowering it enough to allow the reactants to react more easily. Some negative catalysts or inhibitors can do the same by increasing the activation energy.

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3 years ago

A solution contains an unknown amount of dissolved magnesium. Addition of

Scrat [10]

Taking into account the reaction stoichiometry, 2.13 grams of magnesium was dissolved in the solution.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

Mg²⁺(aq) + Na₂CO₃(aq) → MgCO₃(s) + 2 Na⁺(aq)

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Mg²⁺: 1 mole
Na₂CO₃: 1 mole
MgCO₃: 1 mole
Na⁺: 2 moles

The molar mass of the compounds is:

Mg²⁺: 24.3 g/mole
Na₂CO₃: 106 g/mole
MgCO₃: 84.3 g/mole
Na⁺: 23 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

Mg²⁺: 1 mole ×24.3 g/mole= 24.3 grams
Na₂CO₃: 1 mole ×106 g/mole= 106 grams
MgCO₃: 1 mole ×84.3 g/mole=84.3 grams
Na⁺: 2 moles ×23 g/mole= 46 grams

<h3>Mass of magnesium dissolved</h3>

The following rule of three can be applied: If by reaction stoichiometry 1 mole of Na₂CO₃ react with 24.3 grams of magnesium, 0.0877 moles of Na₂CO₃ react with how much mass of magnesium?

$mass of magnesium=\frac{0.0877 moles of Na_{2}C O_{3}x24.3 grams of magnesium }{1 mole of Na_{2}C O_{3}}$

mass of magnesium= 2.13 grams

Finally, 2.13 grams of magnesium was dissolved in the solution.

Learn more about the reaction stoichiometry:

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4 0

3 years ago

Arterial blood contains about 0.25 g of oxygen per liter at 37°C and standard atmospheric pressure. Under these conditions, the

Olin [163]

Firstly we need to determine the partial pressure of O2:

$\begin{gathered} P_{O_2}=X\times P_T \\ P_{O_2}:partial\text{ }pressure \\ X:mole\text{ }fraction \\ P_T:total\text{ }pressure \\ \\ P_{O_2}=0.209\times0.35\text{ }atm \\ P_{O_2}=0.073\text{ }atm \end{gathered}$

We will now use the Henry's Law equation to determine the solubility of the gas:

$\begin{gathered} c=K_H\times P_{O_2} \\ c:solubility\text{ }or\text{ }concentration\text{ }of\text{ }the\text{ }gas(M) \\ K_H:Henry^{\prime}sLawconstant=3.7\times10^{-2}M\text{ }atm^{-1} \\ P_{O_2}:partial\text{ }pressure\text{ }of\text{ }the\text{ }gas=0.073atm \\ \\ c=3.7\times10^{-2}M\text{ }atm^{-1}\times0.073 \\ c=2.7\times10^{-3}M \end{gathered}$

Answer: Solubility is 2.7x10^-3 M

6 0

1 year ago

A buffer solution contains 0.345 M acetic acid and 0.377 M sodium acetate . If 0.0613 moles of potassium hydroxide are added to

melamori03 [73]

Answer:

pH = 5.54

Explanation:

The pH of a buffer solution is given by the Henderson-Hasselbach (H-H) equation:

pH = pKa + log $\frac{[CH_3COO^-]}{[CH_3COOH]}$

For acetic acid, pKa = 4.75.

We calculate the original number of moles for acetic acid and acetate, using the given concentrations and volume:

CH₃COO⁻ ⇒ 0.377 M * 0.250 L = 0.0942 mol CH₃COO⁻

CH₃COOH ⇒ 0.345 M * 0.250 L = 0.0862 mol CH₃COOH

The number of CH₃COO⁻ moles will increase with the added moles of KOH while the number of CH₃COOH moles will decrease by the same amount.

Now we use the H-H equation to calculate the new pH, by using the new concentrations:

pH = 4.75 + log $\frac{(0.0942+0.0613)mol/0.250L}{(0.0862-0.0613)mol/0.250L}$ = 5.54

6 0

3 years ago