The leaves of the rhubarb plant contain high concentrations of diprotic oxalic acid (hooccooh) and must be removed before the stems are used to make rhubarb pie. if pka1 = 1.23 and pka2 = 4.19, what is the ph of a 0.0269 m solution of oxalic acid?

Answers

Answer 1

Answer: Chemical reaction (dissociation) 1: C₂O₄H₂(aq) ⇄ C₂O₄H⁻(aq) + H⁺(aq).
Chemical reaction (dissociation) 2: C₂O₄H⁻(aq) ⇄ C₂O₄²⁻(aq) + H⁺(aq).
c(C₂O₄H⁻) = c(H⁺) = x.
c(C₂O₄H₂) = 0.0269 M.
pKa₁ = 1.23.
Ka₁ = 10∧(-1.23) = 0.059.
Ka₁ = c(C₂O₄H⁻) · c(H⁺) / c(C₂O₄H₂).
0.059 = x² / (0.0269 M - x).
Solve quadratic eqaution: x = c(H⁺) = 0.02 M.
pH = -log(0.02 M) = 1.7.

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The information below describes a redox reaction.Cr3+(aq)+2Cl-(aq)---->Cr(s)+Cl2(s)
2Cl-(aq)--->Cl2(g)+2e-
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What is the final, balanced equation for this reaction?
1.) 2cr3+(aq)+6Cl-(aq) ------> 2Cr(s)+3Cl2(g)
2.) 2Cr3(aq)+2Cl-(aq)+6e- --->Cl2(g)+2Cr(s)
3.) Cr3+(aq)+6Cl-(aq)+3e- ---->2Cr(g)+3Cl2(g)
4.) Cr3+(aq)+2Cl-(aq)------>Cr(s)+Cl2(g)

Answers

Answer: option 1) 2Cr3+(aq)+6Cl-(aq) ------> 2Cr(s)+3Cl2(g)

Explanation:

1) Write the oxidation half-reaction:

$2Cl^-(aq)---\ \textgreater \ Cl_2(g)+2e^-$

2) Write the reduction half-raction:

$Cr^(3+)(aq)+3e^(-)---\ \textgreater \ Cr(s)$

3) Multiply each half-reaction by the appropiate coefficient to equal the number of electrons of both half-reactions.

$6Cl^(-)(aq)---\ \textgreater \ 3Cl_2(g)+6e^(-) 2Cr^(3+)(aq)+6e^(-)---\ \textgreater \ 2Cr(s)$

4) Add both half-reactions

$2Cr^(3+)+6Cl^(-)(aq)---\ \textgreater \ 2Cr(s) +3Cl_2(g)$

And that is the answer. You can count the atoms and charges on every side and check they are equal.

Answer:

Explanation:

got it correct on edge

Select the missing words to complete the definition of buffer capacity. Buffer capacity is the _____________ of acid or base a buffer can handle before pushing the _____________ outside of the buffer range.

Answers

Final answer:

Buffer capacity denotes how much acid or base a buffer solution can integrate before alterations in pH becomes significant. It is crucial in maintaining physiological activities, particularly in blood pH regulation. The substance absorbing the ions is typically a weak acid/base and their conjugates.

Explanation:

Buffer capacity is the amount of acid or base a buffer solution can accommodate before the pH is significantly pushed outside of the buffer range. Solutions that contain sizable quantities of a weak conjugate acid-base pair are known as buffer solutions. These usually experience only slight changes in pH when small amounts of acid or base are added.

A large enough addition of these substances can exceed the buffer capacity, consuming most of the conjugate pair and leading to a drastic change in pH. In living organisms, a variety of buffering systems exist to maintain the pH of blood and other fluids within a strict range between pH 7.35 and 7.45, ensuring normal physiological functioning.

The substance that absorbs the ions is usually a weak acid, which absorbs hydroxyl ions, or a weak concentrate base, which absorbs hydrogen ions. The buffer capacity is greater in solutions that contain more of this weak acid/base and their conjugates.

Learn more about Buffer Capacity here:

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Final answer:

Buffer capacity refers to the amount of acid or base that a buffer solution can absorb before experiencing a significant shift in pH, commonly by one pH unit.

Explanation:

Buffer capacity is the amount of acid or base a buffer can handle before pushing the pH outside of the buffer range. Essentially, it is a measure of a buffer's resistance to pH change upon the addition of an acid or base. Buffer capacity depends on the concentrations of the weak acid and its conjugate base present in the mixture. For instance, a solution with higher concentrations of acetic acid and sodium acetate will have a greater buffer capacity than a more dilute solution of the same components. The buffer's capacity is directly proportional to its ability to absorb strong acids or bases before there's a significant change in pH, typically defined as a shift by one pH unit.

Learn more about Buffer Capacity here:

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I have always enjoyed eating tuna fish. Unfortunately,a study of the mercury content of canned tuna in 2010 foundthat chunk white tuna contains 0.6 ppm Hg and chunk lighttuna contains 0.14 ppm. (S. L. Gerstenberger, A. Martinson,and J. L. Kramer, Environ. Toxicol. Chem. 2010, 29, 237.) TheU.S. Environmental Protection Agency recommends no morethan 0.1 mg Hg/kg body weight per day. I weigh 68 kg. Howoften may I eat a can containing 6 ounces (1 lb 5 16 oz) ofchunk white tuna so that I do not average more than 0.1 mgHg/kg body weight per day? If I switch to chunk light tuna,how often may I eat one can?

Answers

Answer:

You can eat one chunk white tuna of 6 oz every 21,5 minutes

And, you can eat one chunk linght tuna of 6 oz every 5 minutes

Explanation:

The exposure to mercury may cause serious health problems, and is a threat to the development of the child in utero and early in life.

If you weight 68 kg you can eat:

68 kg * 0,1mgHg/ kg = 6,8 mg Hg per day

Chunk white tuna contains 0,6 mg Hg/kg

Thus, you can eat:

6,8 mg Hg * 1 kg tuna/ 0,6 mg Hg = 11,33 kg of chunk white tuna per day

In ounces:

11,33 kg * 35,274oz/ 1 kg = 400 oz per day

You can eat 66,7 6 ounces of chunk white tuna per day. One every 21,5 minutes

Chunk light tuna contains 0,14 mg Hg/kg

Thus, you can eat:

6,8 mg Hg * 1 kg tuna/ 0,14 mg Hg = 48,57 kg of chunk white tuna per day

In ounces:

48,57 kg * 35,274oz/ 1 kg = 1713 oz per day

You can eat 285,6 6 ounces of chunk white tuna per day. One every 5 minutes

I hope it helps!

How many molecules are in 4.27 mol of SiH4

Answers

Answer:

2.57 × 10²⁴ molecules

Explanation:

The number of molecules can be found by using the formula

N = n × L

where n is the number of moles

N is the number of entities

L is the Avogadro's constant which is

6.02 × 10²³ entities

From the question we have

N = 4.27 × 6.02 × 10²³

We have the final answer as

2.57 × 10²⁴ molecules

Hope this helps you

What is a characteristic of property acids pls help

Answers

Answer:

General Characteristics of Acids:

Sour taste (though you should never use this characteristic to identify an acid in the lab) Reacts with a metal to form hydrogen gas. Increases the H+ concentration in water. Donates H+ ions. Turns blue litmus indicator red.

ph>7
also turns blue litmus red

2 N H 3 ( g ) ⟷ N 2 ( g ) + 3 H 2 ( g ) K p = 0.83 Consider your answers above, if the initial pressures for all three species is 1 atm what is the equilibrium pressure of H2? (Hint: Your quadratic will have two solutions, which one is impossible?)