Describe and explain the two situations in which pH can have an appreciable effect on the aqueous solubility of ionic compounds.

Q: What is the strategy to calculate how the pH of the buffer responds to the addition of a strong acid…

A: The strategy used to calculate the pH of the buffer responds to the addition of a strong acid or a…

Q: A 1.34 L buffer solution consists of 0.174 M butanoic acid and 0.250 M sodium butanoate. Calculate…

A: The pH scale is given by the scientist Sorensen in order to express the [H3O+] ion of a solution. It…

Q: Differentiate the carbonate buffer and phosphate buffer systems in terms of pH and pKa. Give…

A: Difference between the carbonate and phosphate buffer is given below and also function of each…

Q: A buffer solution contains 0.340 M ammonium chloride and 0.203 M ammonia. If 0.0488 moles of sodium…

A: To calculate the pH of the buffer solution after adding NaOH solution , we would first calculate the…

Q: write the expression for K, and K, for the reaction PH,BCh(s) = PH:(B) + BCI(B) 1.

A:

Q: What are the main groups in the general qualitative analysis scheme described in this chapter?…

A: Qualitative analysis- It is the ideal analysis of inorganic mixtures to detect basic radicals and…

Q: Investigate some of the factors that affect solubility, including the common-ion effect and the…

A: The process of a solute getting dissolved in a solvent is called dissolution. It is governed by…

Q: A 1.46 L buffer solution consists of 0.171 M butanoic acid and 0.341 M sodium butanoate. Calculate…

A: Given,  Volume of the buffer = 1.46 L  Molarity of butanoic acid = [Butanoic acid] = 0.171 M…

Q: alt. Because the protein solubility depends on the total ion conce alts yielding doubly charged ions…

A: Mass of NaCl = 67.1 gram Moles of NaCl = mass/molar mass = 67.1 gram /58.44 g/mol = 1.148 mol NaCl…

Q: Write the solubility product constant expressions for the following salts: a. SrF2 b. Ag2CrO4 c. HgS…

A:

Q: Lead antimonate, Pb3(SbO4)2, is used as an orange pigment in oil-based paints and in glazes. Write a…

A: Dissolution is the process by which any solid liquid and gaseous substance dissolve in solvent. And…

Q: What is the common ion effect and how does it affect the solubility of an ionic compound?

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Q: Determine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M…

A:

Q: Why do we omit the concentrations of solids and liquids fromequilibrium expressions?

A: The equilibrium constant expression is dependent only on the species which changes significantly and…

Q: Describe how you can increase the buffering capacity of a 0.1 M acetate buffer

A: To give the method to increases the buffering capacity of a 0.1 M acetate buffer.

Q: Why might the actual pH of a prepared buffer deviate from its theoretical pH obtained using the…

A: Henderson-Hasselbalch equation for acid buffer is,  pH=pKa + log[salt][acid]

Q: A 1.32 L buffer solution consists of 0.178 M butanoic acid and 0.349 M sodium butanoate. Calculate…

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Q: Write the solubility product expression for Ag3PO4

A: The solubility reaction of Ag3PO4 is  Ag3PO4 (s) -------> 3 Ag+ (aq) + PO43- (aq)

Q: To an aqueous solution originally containing 1.0 x 10^-4 mol/L Ag+ was added enough of the weak acid…

A: Precipitation of AgCN occurs when the product of concentrations of ions formed equals Ksp. Ksp is…

Q: A 1.49 L buffer solution consists of 0.142 M butanoic acid and 0.286 M sodium butanoate. Calculate…

A: Given: Volume of buffer solution = 1.49 L The concentration of butanoic acid, (HA) = 0.142 M…

Q: A buffer solution contains 0.476 M ammonium bromide and 0.339 M ammonia. If 0.0340 moles of…

A:

Q: The capacity of a buffer towards bases depends upon ... Multiple Choice the strength of the acid…

A: Solution :             Buffer capacity is defined as the efficiency of buffer to resist the change…

Q: c) What is the pH of the groundwater sample in which dichromate is óxidi2e ethanol, which is…

A: The dichromate ion present in a ground water sample is getting oxidized to chromic ion by ethanol…

Q: Write the net ionic equation in which the slightly soluble salt magnesium oxalate, MgC2O4, dissolves…

A: An equation which involves only those species which are involved in the reaction is referred to as a…

Q: What will be the molar solubility of thallium(I) sulfide?

A: Ksp of Tl2S = 6.0x10-22

Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…

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Q: If a solution contains either Pb2+ (aq) or Ag+(aq), how can temperature be manipulated to help…

A: Pb2+ (aq) and Ag+ (aq) belong to the Group I radical, where the group reagent used to detect the…

Q: A 25.5 mL sample of 0.362 M triethylamine, (C2H5)3N, is titrated with 0.285 M hydroiodic acid.…

A: Given data,Molarity of triethylamine=0.362MVolume of triethylamine=25.5mL=0.0255LMolarity of…

Q: Write the K, expression for the dissolution process.

A: Solubility product: It is defined as the product of its dissolved ion concentrations raised to the…

Q: Complete the following solubility constant expression for CaF2. Ksp =

A: The solubility constant expression for CaF2, can be written by writting its balanced equation   so…

Q: The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

Q: Give the solubility-product-constant expressions and Ksp values for barium carbonate.

A: Given BaCO3 Balance equation:                               BaCO3(s)   ⇔          Ba2+(aq)   +…

Q: What is the effect of dilution on the pH of a buffer and the buffer’s capacity? explain

A: When we dilute the solution, the concentration of the substance will decrease.

Q: How many moles of sodium hydroxide would have to be added to 125 mL of a 0.376 M hydrocyanic acid…

A: Ka of HCN = 6.2 × 10-10 pka = -log(ka) = 9.2

Q: If 4.5 moles of nitric acid falls into 8000 L of pure water, what will be the change of the pH of…

A: concentration = mole / litre concentration  = 4.5/8000L                         [ H+]= 0.5625 × 10-3…

Q: What is the effect of concentration of the weak acid on pH of the buffer solution? Explain.

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Q: A 28.3 ml sample of 0.375 M diethylamine, (C,H5)2NH, is titrated with 0.270 M nitric acid. After…

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Q: What is the Kep expression (in terms of molar solubility) for thallium (0 chromate (Tl,CrO,)?

A: Solubility product (Ksp) is defined as the maximum product of the activities or ionic concentrations…

Q: Describe the types and regions of buffers that can occur in a strong acid and weak base titration.…

A: Explained as follows

Q: A 1.48 L buffer solution consists of 0.128 M butanoic acid and 0.338 M sodium butanoate. Calculate…

A:

Q: A 1.43 L buffer solution consists of 0.179 M butanoic acid and 0.300 M sodium butanoate. Calculate…

A: The pH of an acidic buffer can be calculated by using Henderson equation pH = pka + log10…

Q: Explain the role of a buffer, such as an antacid table or sodium bicarbonate, on the pH of a…

A: The antacids play an important role in controlling the pH of the body solution (like blood).…

Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.115 M solution…

A: Given data contains, Volume of solution = 100 mL = 0.100 L [CH3COOH] = 0.115 M pH of the solution =…

Q: how does buffer capacity change with added acid or base?

A: Buffer solution: An aqueous solution consisting of mixture of weak base and its conjugate acid, or…

Q: A buffer is able to resist large changes in pH, because...

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Q: A 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate…

A:

Q: For which of the following aqueous solutions will a decrease of pH increase the solubility? A) CaCO₃…

A: The solution with lower pH means that the higher concentration of hydrogen in the solution. The…

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.