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Concentration Of CN- In 0.1 M HCN Is (Ka = 4*10-10)
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The Degree Of Dissociation Of 0.1 M HCN Solution Is 0.01%. Its Ionisation Constant Would Be
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In Which Of The Following Dissociation Of NH4OH Will Be Minimum
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Ammonium Hydroxide Is A Weak Base Because
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Dissociation Constant Of A Weak Acid Is Decreased By
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An Electrolyte
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Which Will Not Affect The Degree Of Ionization
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The Values Of Dissociation Constants Of Same Acid (at 25° C) Are As Follows. Indicate Which Is The Strongest Acid In Water
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The Colour Of An Electrolyte Solution Depends On
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Theory Of Ionization Was Given By
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A Weak Monobasic Acid Is 1% Ionized In 0.1 M Solution At 25°C. The Percentage Of Ionization In Its 0.025 M Solution Is
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For A Concentrated Solution Of A Weak Electrolyte AxBy Of Concentration C, The Degree Of Dissociation α Is Given As
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Ionisation Depends Upon
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Which Of The Following Is Non - Electrolyte
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Acetic Acid Is A Weak Electrolyte Because
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Chemical Equations Convey Quantitative Information On The
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Theory Of Active Mass Indicates That The Rate Of Chemical Reaction Is Directly Proportional To The
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The Law Of Mass Action Was Enunciated By
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Which Is The False
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Under A Given Set Of Experimental Conditions, With Increase In The Concentration Of The Reactants, The Rate Of A Chemical Reaction
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