Answer:water self-ionize to form an equilibrium system that has [h30+]=1.0x10^-7 M
Explanation:
In a solution that is 90% ethyl alcohol and 10% water, the solute is 10 g and the solvent is 90 g.
given that :
The solute in the solution by mass percent = 10 %
mass percent = ( mass of solute / mass of solution ) × 100%
mass of solute in the solution is = 10 g
The solvent present in solution by mass percent = 90 %
the mass of solvent in the solution is is 90 g
Thus, In a solution that is 90% ethyl alcohol and 10% water, the solute is 10 g and the solvent is 90 g.
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Answer:
E°red for Tl³⁺(aq) | Tl⁺(aq) is 0.78 V
Explanation:
According to cell reaction we can predict which one cathode half cell and which one anode.
We know left hand side electrode where oxidation occur acts as an anode and right hand side electrode where reduction take place acts as an cathode.
Hence Cr²⁺ converted into Cr³⁺ since oxidation is take place where as Ti³⁺ converted into Ti⁺ means reduction take place.
<u>Anode half cell </u>is Cr³⁺(aq) | Cr²⁺(aq) is E⁰red = -0.41 V
<u>Cathode half cell</u> is Ti³⁺(aq) | Ti⁺(aq) is E⁰red = ?
E⁰cell = E⁰cathode - E⁰anode
⇒ E⁰cathode = E⁰cell + E⁰anode
⇒ E⁰cathode = 1.19 + (- 0.41) volt = 0.78 V
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The molarity of the aqueous acid solution : 0.0101 M
<h3>Further explanation </h3>
Titration is a procedure for determining the concentration of a solution by reacting with another solution that is known to be concentrated (usually a standard solution). Determination of the endpoint/equivalence point of the reaction can use indicators according to the appropriate pH range
Acid-base titration formula
Ma. Va. na = Mb. Vb. nb
Ma, Mb = acid base concentration
Va, Vb = acid base volume
na, nb = acid base valence (amount of H⁺, OH⁻)
Va=12.5 ml
na = 2 (H₂SO₄⇒2H⁺+SO₄²⁻⇒2 ion H⁺)
Mb=0.015
Vb=16.8 ml
nb = 1(LiOH⇒Li⁺+OH⁻⇒1 ion OH⁻)
The molarity of the acid(Ma) :
![\tt Ma\times 12.5\times 2=0.015\times 16.8\times 1\\\\Ma=\dfrac{0.015\times 16.8\times 1}{12.5\times 2}\\\\Ma=0.0101](https://tex.z-dn.net/?f=%5Ctt%20Ma%5Ctimes%2012.5%5Ctimes%202%3D0.015%5Ctimes%2016.8%5Ctimes%201%5C%5C%5C%5CMa%3D%5Cdfrac%7B0.015%5Ctimes%2016.8%5Ctimes%201%7D%7B12.5%5Ctimes%202%7D%5C%5C%5C%5CMa%3D0.0101)