Answer:
Explanation:
We are given that 25 mL of 0.10 M is titrated with 0.10 M NaOH(aq).
We have to find the pH of solution
Volume of
Volume of NaoH=0.01 L
Volume of solution =25 +10=35 mL=
Because 1 L=1000 mL
Molarity of NaOH=Concentration OH-=0.10M
Concentration of H+= Molarity of =0.10 M
Number of moles of H+=Molarity multiply by volume of given acid
Number of moles of H+==0.0025 moles
Number of moles of =0.001mole
Number of moles of H+ remaining after adding 10 mL base = 0.0025-0.001=0.0015 moles
Concentration of H+=
pH=-log [H+]=-log [4.28]=-log4.28+2 log 10=-0.631+2
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Answer:
a.
b. K = 192.9
c. Products are favored.
Explanation:
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a. In this case, according to the unbalanced chemical reaction we need to balance HCl as shown below:
In order to reach 2 hydrogen and chlorine atoms at both sides.
b. Here, given the concentrations at equilibrium and the following equilibrium expression, we have:
Therefore, we plug in the data to obtain:
c. Finally, we infer that since K>>1 the forward reaction towards products is favored.
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The reagent which limits the reaction is called limiting reagents.
____
For example:- N2+3H2gives 2NH3.so here nitrogen limits the reaction.
Option B is correct,
With increase in concentration the density of reactants increases and the system becomes more crowded, the greater the reactants will come in contact with each other and collisions occur. If collision is in proper orientation and has optimum energy then its fruitful and yields product. So, the greater the number of reactants, the greater will be the chances of collision and the greater will be the production of products per unit time and hence, greater is the rate of reaction.