An aqueous solution at 25 °C has a pH of 7.13. Calculate the pOH. Round your answer to 2 decimal places.

Q: pH of pure water

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Q: 9. Sketch a titration curve for the titration of 0.100M NH3 (weak base) with 0,100 M HCI. Label the…

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Q: C(s, graphite) + CO(g) + H,(g) - (3)0'H ASixn J/mol·K = N,(g) + 3 H, (g) → 2 NH,(g) ASixn = J/mol·K

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Q: The Ksp for CdCO3 at a certain temperature is equal to 5.51x10-12. What is the molar solubility of…

A: In this question we have to tell the molar solubility of CdCO3 .

Q: Enter your answer in the provided box. Calculate the pH of a 0.43 M KOH solution. pH

A: In this question we have to tell the PH of the 0.43M KOH solution.

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A: The question can be answered by observing the dissociation pattern of acid as well as additive.

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Q: Calculate the energ -1 ,-1

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A: In this question we have to tell the name of the step of the given reaction .

Q: ? 6.

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Q: e chemical formula of the following complex ions.

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Q: 6. If the same amount of heat is added to 25.0 g sample of each of the metals in the chart below,…

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Q: Br MeO MeO Me

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Q: What's the equilibrium expression for the electrochemical cell w/ the shorthand :Mo│MoO2(aq),…

A: Given the shorthand notation of the electrochemical cell is: Mo(s)│MoO2(aq), H+(aq)││RuO4 (aq),…

Q: Calculate the pOH of the following solutions at 25°C. (a) [OH]-8.47 x 10-11 %3D РОН %3D (b) [OH ]=…

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Q: CH3OH(aq)  +  H+(aq)  ⇋  CH3OH2+(aq)  CH3OH2+(aq) + Br-(aq)  → CH3Br(aq)  + H2O(l) which species…

A: Given :-  Step 1  CH3OH(aq)  +  H+(aq)  ⇋  CH3OH2+(aq)  Step 2  CH3OH2+(aq) + Br-(aq)  → CH3Br(aq)…

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Q: Ho,

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Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

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Q: 6. For these reactants: (a) Identify the E+, LG, Nu:. (b) Predict the product(s). (c) Is the…

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Q: When 634. mg of a certain molecular compound X are dissolved in 60. g of cyclohexane (C,H,2), the…

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Q: Me N. Meo OMe MeN- MeN- H...) -N- MeN- Br MeCN, 100 °C NaH, THF; Br H then 6M HCI MeO2C, -Me Me…

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Q: Michael Reaction → 1,5-diketone |. NaO at, acetone 2. 3. H30+, heat

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Q: 3 Consider the following samples of gases: -He N2 (i) (ii) (iii) If all three samples are at the…

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Q: Calculate the standard potential for the cell.

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Q: A 100 ml of 0.100 M phosphate buffer solution with a pH of 8.10 is to be prepared by adding 1.00 M…

A: The required pH of the buffer is 8.10, which is closest to the pKa2 value. H2PO4(aq) ⇌ HPO4-(aq) +…

Q: Part A A 1.0 L buffer solution is 0.250 M HC,H3O, and 0.040 M NaC,H3O,. Which of the following…

A: 6

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Q: Rank the following ionic solids in terms of increasing solubility in water. I. CdF2 (Ksp = 6.44 x…

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Q: enthalpy change

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Q: 2) Find the activity coefficients for both ions of AgCN in a 500 mL solution saturated with AgCN(s)…

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Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.