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3 years ago

During a titration, a known concentration of _ is added to a _ of an unknown concentration g

Chemistry

1 answer:

Vanyuwa [196]3 years ago

8 0

Explanation:

The whole process of titration involves finding the concentration of a solution (usually an acid or base) by adding (titrating) it to a solution(acid or base) with a known concentration.

The solution of unknown concentration (the analyte) is usually placed in an flask, while the solution of known concentration (titrant) is placed in a burette and slowly added to the flask.

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A hydrogen electron is elevated from level 1 to level 2. Another electron is elevated from level 2 to level 4. The transition re

mario62 [17]

the 2to 4 transition is bigger

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3 years ago

Read 2 more answers

If you did not use a watch glass to cover your stock iodine solution, and the concentration of iodine decreased over the course

anygoal [31]

Answer::

<u><em>Lower rate of reaction</em></u>

Explanation:

Lower concentration of reactant in an experiment is indicative of fewer ions or atoms present, which means a slower rate of reaction. In a titration reaction for instance, the end point would take longer to be substantiated, thereby increasing volume of titres. This is further backed up by collision theory which states that more particles in a system improves combinations of molecules.

This however may not be the case if the iodine in question is catalyst, in which case the change in concentration has no effect whatsoever on the reaction rte.

I hope this explanation fits the brief.

5 0

3 years ago

When silver nitrate is added to an aqueous solution of magnesium chloride, a precipitation reaction occurs that produces silver

slavikrds [6]

Answer:

$m_{AgCl}=64.13gAgCl$

Explanation:

Hello,

In this case, the undergone chemical reaction turns out:

$2AgNO_3+MgCl_2-->2AgCl+Mg(NO_3)_2$

In such a way, based on the reacting 21.3 g of magnesium chloride that are consumed the following stoichiometric procedure leads to the required grams of solver chloride precipitate consider their 1 to 2 mole relationship respectively:

$m_{AgCl}=21.3gMgCl_2*\frac{1molMgCl_2}{95.211gMgCl_2}*\frac{2molAgCl}{1molMgCl_2}*\frac{143.32gAgCl}{1molAgCl}=64.13gAgCl$

Best regards.

7 0

4 years ago

How many moles in 34.2 g of sulfur?

BigorU [14]

1.07 mol would be your answer

7 0

4 years ago

Two solutions, initially at 24.69°C, are mixed in a coffee cup calorimeter (Ccal = 105.5 J/°C). When a 200.0 mL volume of 0.100

Lana71 [14]

Answer:The correct answer is option c.

Explanation:

$AgNO_3+NaCl\rightarrow AgCl+NaNO_3$

Specific heat of water = 4.18 J/g°C

Density of water = 1 g/ml

Mass of $AgNO_3$ solution ,m'= $1 g/ml\times 200 ml= 200 g$

Mass of $NaCl$ solution ,m''= $1 g/ml\times 100 ml= 100 g$

Since NaCl solution is present in lessor mass so, it will act limiting reagent.

Heat absorbed by the solution

$Q=mc\Delta T=(m'+m'')c\Delta T=300 g\times 4.18 J/g^oC\times (0.47^oC)=589.38 J$

Heat absorbed by the calorimeter , $Q'=mc'\Delta T=c'\Delta T=105.5J/^oC\times (0.47^oC)=49.585 J$

Heat released during reaction, $\Delta H_{rxn}$ =49.585 J+589.38 J=638.965 J

As we know that NaCl is present as limiting reagent, the product will form according to the availability of NaCl.

Moles of NaCl in 100.0 ml of 0.100 solution = 0.01 moles

1 mol of NaCl gives 1 mol of AgCl, then 0.01 mol of NaCl will give 0.01 mol of AgCl

Heat of the reaction per 1 mol of AgCl = $\frac{638.965 J}{0.01 mol}=6 63896.5 J/mol= 63.896 kJ/mol\approx 64 kJ/mol$

The heat released during the reaction that exothermic reaction's $\Delta H_{rxn}$ is negative.

Hence the correct answer is option c.

5 0

3 years ago

During a titration, a known concentration of _____ is added to a _____ of an unknown concentration g

During a titration, a known concentration of _ is added to a _ of an unknown concentration g