What is the pH of a solution made by dissolving 3.41 grams of calcium fluoride in enough water to make 480 mL of solution? The Ka for HF is 6.8x10–4.

Q: What is the pH of a 0.310 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: Recall the expression of pH for weak acid as follows   pH=12pKa-12logC Here HF is a weak acid with…

Q: The weak acid HZ has a Ka of 2.55×10−4. Calculate the pH of 0.040 M HZ.

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Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

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Q: How many moles of NH3 must be dissolved in water to give 622.4 mL of solution with a pH of 11.08? Ko…

A: Given -> Volume of solution= 622.4 ml = 0.6224 L (1L = 1000ml ) pH = 11.08  Kb = 1.8 × 10-5

Q: What is the pH of a solution made by dissolving 7.46 grams of calcium fluoride in enough water to…

A: Given data,Mass of CaF2=7.46gVolume of solution=550mL=0.550LKa for HF=6.8×10-4

Q: Allylamine, C3H5NH2, is a weak base. A 0.46 M aqueous solution of allylamine has a pH of 12.10. What…

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Q: Aspirin, a drug that is used to relieve minor aches and pain, is a weak monoprotic acid. What is the…

A: we know that pH = -log [H+] so -log [H+] = 3.12 [H+] = 0.000758

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Answer: NH4Cl is the salt of weak base and strong acid, therefore its hydrolysis will take place in…

Q: what is the ph of a solution that is 0.100 m in hydrofluoric acid? The Ka of hydrofluoric acid is…

A: Recall the following expression to find pH of the given solution of hydrofluoric acid. Given that…

Q: H3 is a weak base (?b=1.8×10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0293 M methylamine (CH3NH2)…

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Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

Q: Give two different pH values, explain the relative differences in concentration of H+ between the…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

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Q: If the Ka of a monoprotic weak acid is 7.8×10−6, what is the pH of a 0.47 M solution of this acid?

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Q: What is the pH of a 0.330 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: The objective of this question is to calculate the pH of a 0.330 M solution of HF. The Ka value for…

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.34. What is the Ka of the acid?

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Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: What is the pH of a 0.390 M solution of HF (Ka = 6.8 × 10⁻⁴)?

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Q: What is the pH of a 0.480 M solution of HF (Ka = 6.8 × 10⁻⁴)?

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Q: If the Ka of a monoprotic weak acid is 3.7×10−6, what is the pH of a 0.39 M solution of this acid?

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Q: What is the pH of a solution made by dissolving 6.56 grams of calcium fluoride in enough water to…

A: Mass of calcium fluoride = 6.56 gVolume of solution = 730 mlKa for HF = 6.8 * 10-4Ionic equation is…

Q: What is the pH of a 0.440 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A: In an aqueous solution of HF, the dissociation of weak acid HF and autoionization of water takes…

Q: What is the hydroxide ion, pH, and pOH of a solution with a hydrogen ion concentration of 3.25 x…

A: Given:  [H+] = 3.25 x 10-3 M  Kw = 10-14    Since [H+] < 10-7 M so solution is acidic in nature.…

Q: Morphine, C 17H 19NO 3, is often used to control severe post-operative pain. What is the pH of the…

A: Which one of the following is correct answer

Q: What would be the pH of a 6.55 M solution of hydrocyanic acid (HCN)? (Ka of HCN is 6.2x10^-10

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Q: Sodium hypochlorite (NaOCl, 74.44 g/mol) is a common ingredient in household bleach. What is the pH…

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Q: What is the pH of a 0.210 M solution of HF (Ka = 6.8 × 104)?

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Q: he pH of a half-neutralized solution is 1.86. What is the value of [H+] and Ka?

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Q: What is the pH of a solution made by dissolving 7.61 grams of calcium fluoride in enough water to…

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Q: chemist must prepare 200.0 mL of nitric acid solution with a pH of 1.20 at 25 °C. e will do this in…

A: Given that: The volume of nitric acid, V1 = 200 mL pH = 1.20 molarity of nitric acid, stock…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: What is the pH of a solution made by dissolving 3.11 grams of calcium fluoride in enough water to…

A: Given : Mass of calcium fluoride i.e CaF2 dissolved = 3.11 g Volume of solution = 480 mL = 0.480 L…

Q: What is the pH of a solution made by dissolving 8.06 grams of calcium fluoride in enough water to…

A: pH is defined as a scale used to specify the acidity or basicity of an aqueous solution. If a…

Q: What is the pH of a solution made by dissolving 4.61 grams of calcium fluoride in enough water to…

A: Calculate the moles of CaF2: The molar mass of CaF2 is approximately 78.08 g/mol. So, the moles of…

Q: What is the pH of 0.0190 M NaOH?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: If you had the same concentration of NaOH and Ca(OH)2 which one would have the higher pH? Why?…

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Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

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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.