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(a) If a neutral atom, M, becomes positively charged, has it been oxidised or reduced? Explain your answer and write a general equation using M for the neutral atom.
Atom had been reduced.M - e^- = M+ + e^-
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What is the pH of an aqueous solution of 0.006534 M Ba(OH)<sub>2</sub> at 25<sup>o</sup>C? (Give your answer to two decimal places)
[OH−]=0.006534×2=0.0131M⇒pOH=−log(0.0131)=1.88As we know that,pH+pOH=14∴pH=14−pOH=14−1.88=12.12
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Nickel complex with dimethyl glyoxime is soluble in; * neutral solution acidic solution basic solution all of these
neutral solution
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1. an aqueous solution has a pH equal to 2.what do you infer about its acidic and basic character?
2.what is the colour of methylorange i.acidic mediumii.basic medium
1) It is a very low value of pH. As we know, low pH (<7) is observed in acidic conditions, while high pH (>7) is related with basic conditions. So...
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What is the pH of an aqueous solution having a hydronium-ion concentration of 6.83 × 10-3 mol/L? Is the solution acidic or basic?
According to the definition:pH = - log[H3O+]where [H3O+] - concentration of hydronium ions.As a result:pH = -log(6.83 × 10-3) = 2.17As pH < 7, the solution is acidic.
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Is PH 7 acidic, basic or neutral? What affect PH?
pH is a quantitative measure of the acidity or basicity of aqueous or other liquid solutions. pH is defined as the negative log of the hydrogen ion concentration. The range...
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calculate the [H+] and [OH-]as required for each of the following solution at 25 degree celcius and state whether the solution is neutral or acidic
a)1.0x10-5
Kw = [OH-]x[H+] = 1.010-14 [OH-] = 1.0x10-14/[H+] = 1.0x10-14/1.0x10-5 = 1.0x10-9 M Acidic
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What are the [H3O+] concentrations for the following solutions (T = 25°C)?
Acidic:
Basic:
Neutral:
Tthe [H3O+] concentrations for the following solutions (T = 25°C) Acidic more 10^-7 Basic: less 10^-7 Neutral: 10^-7
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Good day,
For the reaction
3A(g)+2B(g)⇌C(g)
Kc= 72.2 at a temperature of 237 ∘C
Calculate the value of Kp
Express your answer numerically.
Thanks
Kp = Kc×(R×T)ΔnThere is 1 mol of gas on the product side of the chemical equation, and there are 3+2=5 mol of gaseous reactants, so Δn = (1-5) = -4...
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Calculate the hydronium concentration of a certain ionization reaction where the hydroxide concentration is determined to be 2.7 x 10-5 M. Identify if the solution is acidic, basic, or neutral.
pOH= -log(OH-) =-log(2.7×10^-5) =4.569pH= 14-pOHpH= 14-4.569 =9.431[H30+]= antilog(-pH) =antilog(-9.431) =3.707×10^-10 MThe solution is basic since pH is 9.431 and the concentration of hydroxide ions is more than that of hydronium.
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