If a saturated solution has a pH of 11.95 at 25 degrees C determine the mass solubility in g/100mL of Ca(OH)2

Q: A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 72.5 mL of 0.375 M H,So,. 4- Calculate the mass of…

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Q: Calculate the pH at the equivalence point for titrating0.200 M solutions of each of the following…

A: (a) Given, The concentration of NaOH solution is 0.200 M The concentration of HBr solution is 0.200…

Q: 6. A solution is prepared by mixing 25.0 mL of 0.300 M KOH with 100 mL of 0.150 M benzoic acid,…

A: Here we are required to find the pH of the solution.

Q: The K, of hydroxylamine, NH,OH, is 1.10 x 108. A buffer solution is prepared by mixing 100.0 mL of a…

A: A buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its…

Q: Calculate the pH of the resulting solution if 0.250 mole of NaOH is added to 500 mL of a buffer…

A: The volume of 1L is equal to 1000 mL. The number of moles (n) of HF is calculated as shown below…

Q: 4) Calculate the pH of a buffer that is 0.012 M C,H5COOH ( Ka= 6.3x10) and 0.033 M NaC6HsCOO.

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Q: Calculate the pH of a solution containing 20 mL of 0.17 M of a weak weak base B OH, like NH,OH, or…

A: 1. Given information: Volume of weak base = 20 mL Volume of strong acid = 16 mL Concentration of…

Q: You mix 15.0 mL of 0.200 M NH4Cl with 15.0 mL of 0.400 M NH3. What is the pH of the resulting…

A: Given: Concentration of NH4Cl = 0.200 M Volume of NH4Cl solution = 15.0 mL = 0.015 L…

Q: Pyridine, C5H5N, is a weak base with Kb = 1.5 × 10-9. What is the pH at the equivalence point when…

A: When an acid reacts with base then there is a formation of salt. If there is strong acid and weak…

Q: A chemistry graduate student is given 250. mL of a 1.10 M trimethylamine ((CH;),N) s solution.…

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Q: Calculate the molar concentration (M) of NaOH if 25.00 mL of NaOH required 36.68 mL of a 0.9500M…

A: Hcl+NaOH---->NaCl+H2O Neutralization reaction  M1V1/n1=M2V2/n2

Q: What is the pH at 25 degrees Celcius of a solution prepared by dissolving 0.0250 mole of sodium…

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Q: An aqueous solution contains 0.447 M dimethylamine ((CH3)2NH). How many mL of 0.246 M…

A: we need to find the volume of 0.246 M perchloric acid added to form the buffer solution with pH…

Q: to the solution containing 8 grams of Ca (OH) 2 in 50 ml of it add 500 ml of solution 0.1 mol HCl…

A: Given,  Mass of Ca(OH)2 = 8 grams Volume of Ca(OH)2 = 50 ml = 0.05 L Volume of HCl = 500 ml = 0.5 L…

Q: 1. A buffer solution is 0.200 M in HC,H;O2, a monoprotic acid, and 0.200 M in NaCH,O2. K, for the…

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Q: 2. Calculate the [H*] and pH in saturated solution of Ba(OH)2 , which contains 3.90 g of Ba(OH)2 per…

A: The dissociation of Ba(OH)2 : Ba(OH)2 ----> Ba2+ + 2OH-   Mass of Ba(OH)2 = 3.90 g  Volume of…

Q: A chemistry graduate student is given 100. mL. of a 0.60M trimethylamine (CH, N: solution.…

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Q: 5. What is the pH at the equivalence point if it requires 32.50 mL of 0.1500 M KOH to completely…

A: According to Le Chatelier’s principle, “When a system experiences any disturbance in the equilibrium…

Q: What is the pH of a solution prepared by mixing 500 mL of 1.5 M HF with 400mL of 1.00 M NaF? The Ka…

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Q: A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COON to 500 mL of a 0.200 M…

A: The no of moles of sodium acetate and acetic acid are as follows:

Q: Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.025 M HCl

A: Answer:- This question is answered by using the simple concept of calculation of ph of a solution…

Q: A saturated solution of magnesium hydroxide is 3.2 × 10¬4 M Mg(OH)2. What are the hydronium ion and…

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Q: Describe how to prepare 1.0 L of buffer solution of pH 5.0, that can tolerate the addition of 0.3…

A: A buffer is a solution that resists the change in pH upon addition of a small amount of an acid (HA)…

Q: In which of these solutions will HNO, ionize less than it does in pure water? (A) 0.10 M NaCl (B)…

A: The reason for less ionization of species in solution is the common ion effect Here the correct…

Q: If a buffer solution is 0.140 M in a weak base (K, = 5.6 x 10-) and 0.400 M in its conjugate acid,…

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Q: 2) The indicator Haln has Ka = 4.5 x 105, Kaz = 4.5 x 10°. H,ln is red, HIn' is blue, In2 is yellow.…

A: Given data:-

Q: Rank the following solutions according to increasing pH: Note: In the mixing of solutions, assume…

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Q: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

A: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

Q: Calculate the pH of a buffer solution made by mixing 300 mL of 0.3M acetic acid, CH;COOH, and 200-mL…

A: A. 4.4  Given that,   Volume of 0.3 M CH3COOH = 300 mL  = 0.3 L Moles of CH3COOH  = 0.3 M× 0.3 L =…

Q: How many grams of dry NH4Cl nned to be added to 2.50 L of a 0.200 M solution of ammonia, NH3, to…

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Q: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

A: Henderson-Hasselbalch equation, Is an equation which shows the relationship between the pH and pOH…

Q: An aqueous solution contains 0.345 M dimethylamine ((CH3)2NH). How many mL of 0.370 M hydroiodic…

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Q: Explain the attachment

A: Given : Concentration of NaCH3COO = 0.20 M Concentration of HCl = 0.200 M Volume of NaCH3COO…

Q: A 50.00-mL portion of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point…

A: The number of moles of OH-, nOH-, in 29.71 mL of 0.01963 M Ba(OH)2 is; 1000 mL=1.0 LnBa(OH)2=0.01963…

Q: A chemistry graduate student is given 250. mL of a 0.80M pyridine (C.H,N) solution. Pyridine is a…

A: Buffer problem and their detailed solution with reference to the question is given in step-2  first…

Q: Calculate the pH of a buffer that is 0.012 M C,H,COOH ( Ka= 6.3x10) and 0.033 M NaC,H;COO.

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Q: An aqueous solution contains 0.329 M methylamine (CH3NH2). How many mL of 0.305 M perchloric acid…

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Q: In what pH range is Al(OH)3 soluble?   I. Low pH II. Neutral pH III. High pH why is it I. and…

A: We have to tell at what pH range Al(OH)3 is soluble. The given options are Low pH Neutral pH High…

Q: A research wishes to prepare a buffer with a pH of 4.74 from weak acid HA (Ka = 2.57 x 105) and the…

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Q: A solution is made by mixing 150mL of 0.12 M HCN, 100 mL of 0.56 M NaOH and 75 mL of 0.78 M HCl.…

A: HCl dissociates into H+ and Cl-. Thus: [HCl] = [H+] Thus [H+] obtained from HCl =0.78 M Calculation…

Q: Suppose you. have 185mL of a buffer that is 0.160 M in both formic acid (HCOOH) and its conjugate…

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Q: 28. K, (Alloxanic acid) = 2.3 x 10 and K, (HF) = 6.8 x 104. Consider the following two aqueous…

A: Given :  Ka (Alloxanic acid) = 2.3 x 10-7  Ka(HF) = 6.8 x 10-4

Q: I mix 100 mL of 0.100 M HCl in 250 mL of 0.150 M NH3.   I add 50.0 mL of 0.0500 M NaOH.   What…

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Q: What is the pH of a 100ml solution formed by adding 0.1mole NaOH to a buffer solution that contains…

A: Added base will neutralize acid and increase amount of the conjugate base salt in solution. Using…

Q: What is the pH of the solution that results from adding 24.7 mL of 0.11 M HCl to 25.2 mL of 0.41 M…

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Q: O Calculate the pH of a buffer that is 0.012 M C6H$COOH ( Ka= 6.3x10³) and 0.033 M NaCgH5COO.

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Q: What mass of NaOH would be added to a one liter 0.200 M solution of acetic acid (pKa = 4.76) to…

A: Given : Volume of solution = 1 L  Concentration of acetic acid = 0.200 M And pH of solution = 4.76…

Q: The K, for NH3 is 1.8 x 10-° at 25°C. Calculate the pH of a buffer solution made by mixing 45.7 mL…

A: Given data:- A buffer solution made by mixing 65.1 mL of 0.142 M NH3 with 38.0 mL of 0.172 M NH4Cl…

Q: 1. A buffer solution is 0.200 M in HC.H,O2, a monoprotic acid, and 0.200 M in NaC,H;O2. K, for the…

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Q: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

A: Buffer is a solution which is formed by mixing of an acid and salt of its conjugate base or base and…

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.