# Where Formic Acid Is Found

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If you are looking for the answer of where formic acid is found, you’ve got the right page. We have approximately 10 FAQ regarding where formic acid is found. Read it below.

## determine the percentage composition of each element in formic acid,

Ask: determine the percentage composition of each element in formic acid, HCOOH​

Formic Acid molecular weight

Molar mass of HCOOH = 46.02538 g/mol

Convert grams Formic Acid to moles  or  moles Formic Acid to grams

Molecular weight calculation:

1.00794 + 12.0107 + 15.9994 + 15.9994 + 1.00794

Percent composition by element

Element   Symbol   Atomic Mass   # of Atoms   Mass Percent

Hydrogen H           1.00794                     2                  4.380%

Carbon          C          12.0107                   1                26.096%

Oxygen            O           15.9994           2              69.524%

## What kind of acid is found in ants? a) acetic

Ask: What kind of acid is found in ants? a) acetic b) formic c) nitric d) glutamic

B.) Formic acid is the answer

## The pH of a 0.10 M solution of formic acid

Ask: The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39. What is the Ka of the acid?​

Explanation:

hope it helps ☺️

## 3. How many grams of formic acid (HCOOH) are contained

Ask: 3. How many grams of formic acid (HCOOH) are contained in 15 L of 22.0% formic acid solution that has a density of 1.15 g/ml?​

13.2 M

Explanation:

The first thing to do here is pick a sample of this solution.

Since you’re going to find its molarity, you can make the calculations easier by picking a

1.00-L

sample. Keep in mind ,the answer will be the same regardless of the volume you pick.

So, use the density of the solution to determine how many grams you get in that respective volume

1.00

L

1000

mL

1

L

1.20 g

1

mL

=

1200 g

Now, you that the percent concentration by mass for this solution is

40.0% HCl

. This means that you get

40.0 g

of hydrochloric acid for every

100.0 g

of solution.

The mass of hydrochloric acid you get in that sample will thus be

1200

g solution

40.0 g HCl

100

g solution

=

480 g HCl

Use hydrochloric acid’s molar mass to determine how many moles you have in that many grams

480

g

1 mole HCl

36.46

g

=

13.17 moles HCl

The molarity of the solution will thus be – remember that we started with a

1.00-L

sample

c

=

n

V

c

=

13.17 moles

1.00 L

=

13.2 M

rounded to three sig figs

SIDE NOTE This is very close to the maximum possible concentration for hydrochloric acid in aqueous solution. At this concentration, the solution is actually fuming at a significant evaporation rate.

## Which of the following is NOT an acid cleanera. oxalic

Ask: Which of the following is NOT an acid cleaner

a. oxalic acid
a. formic acid
b. muriatic acid
c. sulfamic acid​

1. A

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C. Sulfamic acid

Explanation:

That’s all ik

## what is the common name of formic acid ​

Ask: what is the common name of formic acid ​

The most widely used base is sodium methoxide. Hydrolysis of the methyl formate produces formic acid: HCO2CH3 + H2O → HCOOH + CH3OH.

Formic acid, also known as formate or methanoic acid, belongs to the class of organic compounds known as carboxylic acids.

## Formic Acid has a pKa of 4.401. If the solution

Ask: Formic Acid has a pKa of 4.401. If the solution pH is 3.495, what percentage of the acid is undissociated?

Percentage of the acid is undissociated : 87.5%

### Further explanation

pH is the degree of acidity of a solution that depends on the concentration of H ions. The greater the value the more acidic the solution and the smaller the pH.

pH = – log [H⁺]

So that the two quantities between pH and [H⁺] are inversely proportional because they are associated with negative values.

According to Arrhenius, Acid is a compound which in water releases OH-ions

Electrolytes (acids or bases) with a small degree of ionization are classified as weak electrolytes

OH concentration and molarity can be related to the formula

[tex]rm [H ^ +] = sqrt {Ka.M}[/tex]

Ka = acid ionization constant

M = molarity

In a weak acid reaction:

HA —-> H⁺ + A⁻

Ka = acid ionization constant  for this reaction

[tex]rm Ka=dfrac{[H^+][A^-]}{[HA]}[/tex]

Formic Acid has a pKa of 4.401

then :

[tex]rm Ka=10^{-4.401}[/tex]

the solution pH is 3.495

then :

[tex]rm [H^+]=10^{-3.495}[/tex]

Because [ H⁺] =[A⁻] : then

[tex]rm {[H^+]=[A^-]=10^{-3.945}[/tex]

Value of [HA] :

[tex]rm [HA]=dfrac{(10^{-3.495})^2}{10^{-4.401}}\\~[HA]=10^{-2.589}[/tex]

Percent dissociation:

[tex]rm dfrac{[H^+]}{[HA]}=dfrac{10^{-3.495}}{10^{-2.589}}=10^{-0.906}[/tex]

Percent undissociated:

[tex]rm 1-10^{-0.906}=0.875=87.5%[/tex]

pH of a 0.0001M of NaOH

https://brainly.ph/question/2318238

The pH of a solution decreases by 2.0

https://brainly.ph/question/1940382

the pH of a solution

https://brainly.ph/question/2255019

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## what is the classification of Formic acid​

Ask: what is the classification of Formic acid​

classified as acid

Explanation:

hula lang

Explanation:

Formic acid, also known as formate or methanoic acid, belongs to the class of organic compounds known as carboxylic acids. Carboxylic acids are compounds containing a carboxylic acid group with the formula -C(=O)OH. Formic acid exists as a liquid, soluble (in water), and a weakly acidic compound (based on its pKa).

## 15. Below are the types of abrasive cleaners except one.A.

Ask: 15. Below are the types of abrasive cleaners except one.
A. oxalic acid
B. formic acid
C. muriatic acid
D. sulfamic acid​

B formic acid

Explanation:

Formic acid is the simplest carboxylic acid, containing a single carbon. Occurs naturally in various sources including the venom of bee and ant stings, and is a useful organic synthetic reagent. Principally used as a preservative and antibacterial agent in livestock feed.

## which of the following is an amino acid? a. Formic

Ask: which of the following is an amino acid? a. Formic acid b. Glycolic Acid c. Glycerol d. Glycine​

C is the answer on the question

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