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3 years ago

PLEEASE HELP TIMED WILL GIVE BRAINLIEST TO CORRECT ANSWER NLY PLEASEEEE HELPPPP

Chemistry

2 answers:

Arturiano [62]3 years ago

8 0

Answer:

1) 1.15 mol

2) M=0.45

3) 22.5 mL

4) 6.25 mL

Explanation:

550 mL= 0.55 L

M= mol solute/ L solution

mol solute= M * L solution

mol solute= (2.1 M * 0.55 L ) M=1.15 mol solute

155 mL = 0.155 L

80 g -> 1 mol NH4NO3

5.61 g -> x

x= (5.61 g * 1 mol NH4NO3)/80 g x= 0.07 mol NH4NO3

M=(0.07 mol NH4NO3)/0.155 L M=0.45

3) M1V1=M2V2

V1= M2V2/M1

V1= (0.500 M * 0.225 L)/5.00 M V1=0.0225 L =22.5 mL

4) M1V1=M2V2

V1= M2V2/M1

V1= (0.25 M * 0.45 L)/ 18.0 M

V1=6.25 x 10^-3 L = 6.25 mL

Grace [21]3 years ago

6 0

Answer:

Explanation:

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Answer

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Procedure

The Henderson–Hasselbalch equation relates the pH of a chemical solution of a weak acid to the numerical value of the acid dissociation constant, Kₐ. In this equation, [HA] and [A⁻] refer to the equilibrium concentrations of the conjugate acid-base pair used to create the buffer solution.

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