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dangina [55]
3 years ago
8

Which of the following acids is the WEAKEST? The acid is followed by its Ka value.HF, 3.5 × 10^-4HNO2, 4.6 × 10^-4HCN, 4.9 × 10^

-10HCOOH, 1.8 × 10^-4HClO2, 1.1 × 10^-2
Chemistry
1 answer:
Mila [183]3 years ago
4 0

Answer:

HCN

Explanation:

There are several factors that can tell us when an acid is stronger than another, which are the following:

1. The Polarity of the X - H Bond

2. Size of the X atom.

3. Charge on the acid.

4. Oxidation state of the central atom

5. Values of Ka and pKa.

From all of this factors, we can see that the exercise is already giving us values of Ka, and also we have different types of acid, not only with the form H - X

So, we will base the force of an acid by it's pKa value.

The pKa value which is calculated with the expression:

pKa = -logKa

pKa is a value that indicates how strong is the acid you are working with. This value can vary depending on factors such the charge of the acid. I f this charge can be easily distributed in resonance structures, the compound is more acidic, and therefore the pKa value is lower.

The lower the pKa, the more acidic the compound is.

So calculating the pKa on every structure we have:

HF: pKa = -log(3.5x10^-4) = 3.46

HNO2: pKa = -log(4.6x10^-4) = 3.34

HCN: pKa = -log(4.9x10^-10) = 9.31

HCOOH: pKa = -log(1.8x10^-4) = 3.74

HClO2: -log(1.1x10^-2) = 1.96

So according to all this values, we can conclude that the weakest acid is the HCN

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Calculate the volume of 5.0 grams of NO gas at STP.
Sveta_85 [38]

Answer:

The volume of  5.0 g CO  2  is  2.6 L CO  2  at STP

Explanation:

STP

STP is currently  

0

∘

C

or  

273.15 K

, which are equal, though the Kelvin temperature scale is used for gas laws; and pressure is  

10

5

.

Pascals (Pa)

, but most people use  

100 kPa

, which is equal to  

10

5

.

Pa

.

You will use the ideal gas law to answer this question. Its formula is:

P

V

=

n

R

T

,

where  

P

is pressure,  

V

is volume,  

n

is moles,  

R

is a gas constant, and  

T

is temperature in Kelvins.

Determine moles

You may have noticed that the equation requires moles  

(

n

)

, but you have been given the mass of  

CO

2

. To determine moles, you multiply the given mass by the inverse of the molar mass of  

CO

2

, which is  

44.009 g/mol

.

5.0

g CO

2

×

1

mol CO

2

44.009

g CO

2

=

0.1136 mol CO

2

Organize your data

.

Given/Known

P

=

100 kPa

n

=

0.1136 mol

R

=

8.3145 L kPa K

−

1

mol

−

1

https://en.wikipedia.org/wiki/Gas_constant

T

=

273.15 K

Unknown:  

V

Solve for volume using the ideal gas law.

Rearrange the formula to isolate  

V

. Insert your data into the equation and solve.

V

=

n

R

T

P

V

=

0.1136

mol

×

8.3145

.

L

kPa

K

−

1

mol

−

1

×

273.15

K

100

kPa

=

2.6 L CO

2

rounded to two significant figures due to  

5.0 g

Answer link

Doc048

May 18, 2017

I got 2.55 Liters

Explanation:

1 mole of any gas at STP = 22.4 Liters

5

g

C

O

2

(

g

)

=

5

g

44

(

g

mole

)

=

0.114

mole

C

O

2

(

g

)

Volume of 0.114 mole  

C

O

2

(

g

)

= (0.114 mole)(22.4 L/mole) = 2.55 Liters  

C

O

2

(g) at STP

6 0
3 years ago
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