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BCH 100 Study Guide - Final Guide: Programmable Calculator, Hydrogen Bond, Hyperventilation

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silverhorse257
22 Nov 2016
School
UC Riverside
Department
Biochemistry
Course
BCH 100
Professor
Stephanie Dingwall

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Document Summary

Lecture 2: acids, bases, and buffers: terminology (explain or define; understand use of terms): ion product of water, bronsted acid, bronsted base, strong acid, weak acid, conjugate acid-base pair, ph, pka, titration curve, buffer. The equilibrium constant for the dissociation of water into hydroxide and hydronium ions. Kw= [h3o+][oh-], for pure water the value of kw is. Two species that are related by 1 hydrogen ion (h+) ph pka. An experiment in which measured amounts of acid (or base) are added to measured amounts of base (or acid) A solution that resists change in ph: explain the difference between a hydrogen bond donor and a bronsted acid (a proton donor). In hydrogen bonding the hydrogen is positive and is seen as (cid:862)donating(cid:863) a hydrogen to the bond. A bronstead acid is proton donor because is physically releases a hydrogen atom which is then accepted by the base: explain how the [h+] and [oh ] concentrations are related in aqueous solutions.

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Related Questions

QUESTION 1

Which of the following substances is most acidic?

Cow’s milk - pH 6.6

Apple juice - pH 3.0

Tomato juice - pH 4.5

Distilled water - pH 7.0

2 points

QUESTION 2

A buffer is a substance that converts:

Alkaline solutions to neutral solutions.

Acidic solutions to alkaline solutions.

Strong bases or acids to weak bases or acids.

Acidic solutions to neutral solutions.

QUESTION 3

How does a solution of pH 7 compare to a solution of pH 10?

pH 7 has more OH- ions

pH 7 is more basic

pH 7 has a higher pH

pH 7 has more H+ ions

2 points

QUESTION 4

According to the Arrhenius Theory of acids and bases, a base is:

A substance that decrease the amount of hydroxide ions present.

A substance that increases the amount of hydroxide ions present when it is dissolved in water.

A substance that increase the amount of hydrogen ions present.

A substance that increases the amount of hydrogen ions present when it is dissolved in water.

QUESTION 5

Which of the following are true regarding acid-base titrations?

They are used to determine the concentration of an unknown acid or base.

The acid or the base must be a standard solution with a known concentration

The standard solution is titrated into the chemical with the unknown concentration.

All of the above are true regarding acid-base titrations.

2 points

QUESTION 6

Which of the following is not an example of a neutralization reaction?

HCl + NaOH NaCl +H2O

2 NaOH + H2CO3 Na2CO3 +2 H2O

H2SO4 + 2 NH4OH (NH4)2SO4 + 2 H2O

2 AgNO3 + Zn 2Ag +Zn(NO3)2

QUESTION 7

Which acid base theory defines an acid as a proton donor and a base as a proton acceptor?

Arrhenius Theory

Bronsted-Lowery Theory

Conjugate Pairs Theory

Lewis Theory

2 points

QUESTION 8

The Arrhenius Theory states that acid-base reactions create a solution composed of a water and a salt. This is because mixing an acidic and basic solution together yields:

A neutral solution

A solution with a pH at or near 7

Both A and B are correct

QUESTION 9

Which of the following correctly defines a standard solution?

A solution which always has the same molecular geometry.

A solution in which the concentration is precisely known.

A solution in which the volume is precisely known.

A solution which always has different levels of solutes and solvents.

2 points

QUESTION 10

Acids naturally present in food are generally safe to eat because they are usually:

Concentrated

Dilute

Weak

Strong

None of the above are correct

Part A A fuel cell differs from a battery because the current is being generated from a reduction-oxidation (redox) reaction in which the reactant is consumed. A classic example of a fuel cell is the phosphoric acid fuel cell (PAFC), which have been used in stationary power generators, buses, and even submarines. Fuel cells require an electrolyte (similar to batteries) to carry electrically charged species between the electrodes, and a PAFC utilizes phosphoric acid (H3PO4) as its electrolyte. Phosphoric acid has three acidic protons that can dissociate in water, as highlighted in red here: H3PO4. However, it is considered a weak acid because some of the acid will remain in molecular form when dissolved in water. Write the complete ionic equation that depicts the dissociation of the first proton for the weak acid phosphoric acid (H3PO4). Make certain you include all charges for any ions produced. Express you answer as a chemical equation including phases. Titrations as analytical neutralization reactions Neutralization reactions can occur between any combination of weak/strong acids and bases. When we want to determine the concentration of a base in solution, we can apply the concept of neutralization by reacting the base with a known amount of an acid in the presence of an indicator (a compound that changes color depending on the pH). This method of determining the concentration of a base is called acid-base titration, and it can also be used to determine the concentration of an acid by titrating it with a known amount of base. A common acid to use for titrations is potassium hydrogen phthalate (written as KHP or KHPh; do not confuse the P for phosphorus). The reason KHP is common is because it is solid at room temperature, and we can accurately mass the amount that is added to solution. As a soluble salt, KHP completely dissociates to form a potassium ion (K+) and an acidic hydrogen phthalate ion (HP−), which is a weak acid that has only one acidic hydrogen. This ionization is depicted below. KHP(s) → K+(aq)+HP−(aq) Although ionization (the formation of ions) occurs as a result of acid dissociation for most weak acids, KHP ionizes before acid dissociation occurs. In other words, HP− is a weak acid ion. Part C If you wanted to determine how much KOH (potassium hydroxide; a strong base) was dissolved in water, you could titrate it with a known amount of KHP (potassium hydrogen phthalate; a weak acid) until a color change indicates that the base is completely neutralized. The molecular equation below depicts this neutralization reaction. KHP(aq)+KOH(aq)→K2P(aq)+H2O(l) Write the net ionic equation that depicts the neutralization of the base by potassium hydrogen phthalate. Instead of using the entire chemical formula of phthalate, use HP− to represent the acidic hydrogen phthalate ion and P2− to represent the phthalate ion. Express your answer as a net ionic equation including phases.