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3 years ago

How do you identify whether a solution is a buffer solution or not

Chemistry

1 answer:

Leviafan [203]3 years ago

4 0

Answer:

You check whether the PH level changes when you add little amounts of strong acid or base. If you see that there is little to no change in the PH, then it is a buffer solution.

Hope that answers your question

Explanation:

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What is pH when 4.0 mL of 2.0 M barium hydroxide is added to 10.0 mL of 1.00 M nitric acid?

Anika [276]

Answer : The pH of the solution will be 13.63.

Solution:

Moles of hydroxide ions in barium hydroxide solution

$BaOH_2\rightarrow Ba^++2(OH)^-$

Number of moles = (concentration) $\times$ (volume in liters) ...(1)(1L=1000mL)

2.0 M barium hydroxide in solution

Number of moles of $Ba(OH)_2$ in 2.0 M solution $=2.0 M\times 0.004 L=0.008$ moles

If One mole of barium hydroxide gives two moles of hydroxide in solution then 0.008 moles will give:

Number of moles of $OH^-=(2)\times (0.008 mol)=0.016$ moles

Moles of $H^+$ ions in nitric acid

$HNO_3\rightarrow NO^{-}_{3}+H^+$

In 1.00 M nitric acid solution

Moles of nitric acid in 1.0 M solution $=(1.0 M)\times(0.010 L)=0.010$ moles

If one mole of nitric acid will give one moles of $H^+$ ion.

Then 0.010 moles of nitric acid in solution will give :

Number of moles of $H^+=(1)\times (0.010 mol)=0.010$ moles

Since , the reaction will be neutralization reaction, equal number of moles of $H^+$ will neutralize equal number of moles of $OH^-$

So,0.010 moles of $H^+$ will neutralize 0.010 moles of $OH^-$ in the solution

Remaining moles of $OH^-=0.016- 0.01=0.006$ moles

Concentration of $[OH^-]$ resulting solution

Resulting volume of the solution : 0.004 + 0.010 liters

Calculating $[OH^-]$ by using equation (1).

$[OH^-]=\frac{0.006}{0.004L+0.010 L}=0.4285 M$

$pOH=-log[OH^-]=-log(0.4285)=0.367$

$pH=14-pOH=14-0.367=13.633$

The pH of the solution will be 13.633.

8 0

4 years ago

What is water in a scientific knowledge

AleksandrR [38]

water in scientific knowledge is H20

6 0

4 years ago

What is the volume of 6 moles of hydrogen gas, H2 (g)

Yuki888 [10]

Answer:

Molar volume, or volume of one mole of gas , depends on pressure and temperature, and is 22.4 liters - at 0 °C (273.15 K) and 1 atm (101325 Pa), or STP (Standard Temperature and Pressure), for every gas which behaves similarly to an ideal gas. The ideal gas molar volume increases to 24.0 liters as the temperature increases to 20 °C (at 1 atm).

4 0

3 years ago

Consider the following precipitation reaction (balanced). precipitation reaction: 2NH4Br(aq)+Pb(C2H3O2)2(aq)⟶2NH4C2H3O2(aq)+PbBr

sweet [91]

Answer:

Pb2+ (aq) & 2Br- (aq) --> PbBr2 (s).

Explanation:

Equation of the reaction:

Pb(C2H32O2)2 (aq) + 2 NH4Br (aq) --> 2NH4C2H3O2 (aq) + PbBr2 (s)

Ionic equation:

Pb+2(aq) + 2(C2H3O2)-1 (aq) + 2(NH4+) (aq) + 2Br-1 (aq) --> 2(NH4+) (aq) + 2(C2H3O2-) (aq) + PbBr2 (s)

2(NH4)+1(aq) & 2(C2H3O2)-1 (aq) cancel out from both sides, you are left with the net ionic equation :

Pb2+ (aq) & 2Br- (aq) --> PbBr2 (s).

6 0

3 years ago

what is always true of a combustion reaction? oxygen gas must be one of the reactants carbon monoxide will be produced the react

cestrela7 [59]

The correct answer should be
carbon monoxide will be produced

Combustions release heat, they don't absorb it. Oxygen is not necessary as other gasses can also do it, while chlorine is not necessary.

6 0

3 years ago