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The concentrations of fluoride, lead, nitrate and iron in a water sample from an underground lake were found to be 1000 ppb, 40 ppb, 100 ppm and 0.2 ppm, respectively. This water is unsuitable for drinking due to high concentration of
  • a)
    Fluoride
  • b)
    Lead
  • c)
    Nitrate
  • d)
    Iron
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
The concentrations of fluoride, lead, nitrate and iron in a water samp...
Fluoride - 1000 ppb = 1 ppm (which is within the permitted levels, viz. < 10 ppm)
Lead - 40 ppb (which is within the permitted levels, viz. < 50 ppb)
Iron - 0.2 ppm( is the maximum permmiscible limit)
Nitrate - 100 ppm is not suitable for drinking.
[NO3-] > 50 ppm, in drinking water can cause disease such as methemoglobinemia ('blue baby' syndrome).
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Not all chemical reactions proceed to a stage at which the concentrations of the reactants become vanishingly small. Here we consider the kinetics of such reactions.Let a reaction be represented in general terms by the schemewhere k., and k_., represent the rate constants for the forwards and reverse reactions, respectively. The equilibrium constant for this reaction may be written asK = [B] /[A] = K1/K1 --(1)where the subscript 00 refers to a time t, sufficiently long to establish equilibrium at the given temperature. The initial concentration of species A is [A]O, and that of B is [B]O . After a time t, let the concentration of species A be [A/t and that of B be [Bat. The total rate of change of [At is given byd[A]t/dt= - K1[A]t + k-1[B]tIf, as is usual, [B]O is initially zero, it follows from a mass balance that at any time t,[Bat = [A]0 - [A]t, whenced[A]t/dt = K1[A]t + k-1([A]O - [A]t)ord[A]t/dt = (K1 + k-1)For the reaction (having both 1ts order reactions), the concentration as a function of time are given for a certain experimental run along with a tangent to the graph at the origin. The ratio of the magnitude of the slopes of the graph of [A/ and [C/ at the origin would be

Not all chemical reactions proceed to a stage at which the concentrations of the reactants become vanishingly small. Here we consider the kinetics of such reactions.Let a reaction be represented in general terms by the schemewhere k., and k_., represent the rate constants for the forwards and reverse reactions, respectively. The equilibrium constant for this reaction may be written asK = [B] /[A] = K1/K1 --(1)where the subscript 00 refers to a time t, sufficiently long to establish equilibrium at the given temperature. The initial concentration of species A is [A]O, and that of B is [B]O . After a time t, let the concentration of species A be [A/t and that of B be [Bat. The total rate of change of [At is given byd[A]t/dt= - K1[A]t + k-1[B]tIf, as is usual, [B]O is initially zero, it follows from a mass balance that at any time t,[Bat = [A]0 - [A]t, whenced[A]t/dt = K1[A]t + k-1([A]O - [A]t)ord[A]t/dt = (K1 + k-1)At what time is the rate of change of concentration of A equal to rate of change of concentration of C in magnitude ?

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The concentrations of fluoride, lead, nitrate and iron in a water sample from an underground lake were found to be 1000 ppb, 40 ppb, 100 ppm and 0.2 ppm, respectively. This water is unsuitable for drinking due to high concentration ofa)Fluorideb)Leadc)Nitrated)IronCorrect answer is option 'C'. Can you explain this answer?
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