if 65ml of 0.25M naoh are combined with 76ml of 0.3M h2so4 .What is the pH if the solution is diluted to 750 ml

Q: What mass of KOH would need to be dissolved in 500.0 mL of water to produce a solution with a pH of…

A: KOH completely dissociates since it is strong base.Concentration of KOH is determined as follows,

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH  = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: A solution is prepared by diluting 0.55 mol HNO3 with water to a volume of 1.75L. What is the pH of…

A: Molarity = Number of moles of solute/Volume of solution in L pH = -log[H+]

Q: An aqueous solution at 25.0oC contains [H+] = 0.090M. What is the pH of the solution?

A:

Q: What volume (in mL) of 8.84 M HBr would be required to make 300.0 mL of a solution with a pH of…

A:

Q: A solution is made by dissolving 0.06100 moles of Ba(OH)2 in enough water to make 250.0 mL of…

A: Given, moles of Ba(OH)2 = 0.06100 moles Volume of the solution = 250.0 mL = 0.250 L pH of the…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: A 0.632 M solution of a monoprotic base has a pH of 11.53. What is the ionization constant of this…

A: Using pH we will get the consentration of OH-. Now since its a monoprotic base. means it will look…

Q: A solution containing 572.0mL of 0.6300MHCl is diluted to a volume of 1.000L. What is the pH of this…

A:

Q: If the ?bKb of a weak base is 1.5×10−6,1.5×10−6, what is the pH of a 0.34 M0.34 M solution of this…

A:

Q: An aqueous solution contains 5.24x10 M NaHS and 0.132 M H,S. The pH of this solution is

A: pKa1 of H2S = 6.99  Henderson Hassebalch equation : pH =pKa + log [salt]/[acid]

Q: What is the pH and pOH of a solution made by adding water to 15 grams of hydroiodic acid until the…

A:

Q: A solution containing 572.0mL of 0.6309 M HCl is diluted to a volume of 1.000 L. What is the pH of…

A: "pH" is utilized to analyze the quantity of [H+] ion in concentration term in any solution. It…

Q: An aqueous solution at 25 °C is 12.9% HNO, by mass and has a density of 1.049 g/mL. What is the pH…

A: Assuming we have 100 g of solution  hence mass of HNO3 in it = mass % X mass of solution / 100 =…

Q: To increase the pH of 1.50 L of 0.25 M HCIO3 (aq), which of the following would you add to the…

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Q: A solution is prepared by dissolving 0.00050 mol KOH in enough water to prepare 500.0 mL of…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH3NH3* and 0.117…

A: TThe base is the substance that gives OH- or accepts H+ ions in solution. The Henderson Hasselbalch…

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.90. What is the Kb of this…

A: Given: Concentration of base = 0.0910 M And pH of solution = 11.90  Since pOH = 14 - pH => pOH =…

Q: An aqueous solution at 25 ∘C is 14.7% HNO3 by mass and has a density of 1.043 g/mL. What is the pH…

A: The acidity of a solution depends on the concentration of the [H]+ ion. The pH is the most…

Q: An aqueous solution at 25 °C is 8.29% LİOH by mass and has a density of 1.092 g/mL. What is the pH?

A: Assuming we have 100 g of solution  hence mass of LiOH = mass % X mass of solution / 100 = 8.29 X…

Q: The pH of an aqueous solution of 0.353 M aniline (a weak base with the formula C¿H2NH,) is

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

Q: An aqueous solution at 25 °C is 14.4% HNO, by mass and has a density of 1.054 g/mL. What is the pH…

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Q: Diluted sulfuric acid has a density of 1.3 g / ml and contains 39% by mass of H2SO4. a) What is the…

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Q: pH of an aqueous solution of 0.355 M acetylsalicylic acid (aspirin) , HC9H7O4, is .

A:

Q: A solution labeled 5 x 10M HCIO4 has a pH of. Do you see a problem with this answer? Briefly…

A: molarity is defined as  no.of moles of solute devided by volume of solution in liter. Whereas pH is…

Q: Calculate the pH of each of the following strong acid solutions: 5.00 mL of 0.250 M HClO4 diluted to…

A:

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: A 75.00-mL portion of a solution that is 0.0460 M in HClO4 is treated with 150.00 mL of 0.0230 M…

A: Acid reacts with base to form salt and water. The given acid is HClO4 and base is KOH.

Q: Which solution would have the higher pH: 0.010 M HNO2 or 0.010 M HNO3? Explain.

A: pH of any solution is defined as negative logarithm of H3O+ or H+ concentration present in solution…

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

Q: The ?a of a weak monoprotic acid is 1.45×10−5. What is the pH of a 0.0784 M solution of this acid?

A: The weak acid dissociation is written as:

Q: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: A solution is prepared by adding 0.0231 moles of H3O+ ions to 3.33L of water. What is the pH of this…

A: Given : moles of H3O+ ions = 0.0231 mol And volume of solution = volume of water approximately =…

Q: A 0.15 M solution of a certain weak acid has a pH of 4.25. The K, of the weak acid is

A:

Q: A solution of sodium acetate 1NaCH3COO2 has a pH of 9.70. What is the molarity of the solution?

A: pH scale is used to measure the acidity or basicity of the solution. If the solution is acidic in…

Q: The pH of an aqueous KOH solution is 12.38. What is the hydrogen ion concentration of this solution?

A:

Q: A solution is prepared by mixing 0.2 moles of HCl into water until the final volume of the solution…

A: pH = -log[H3O+]  This formula is used to calculate to pH .

Q: A solution containing 175mL of 1.50MHBr is diluted to a volume of 1.00L. What is the pH of this…

A: Given, M1 = 1.50 M V1 = 175 mL V2 = 1.00 L M2 = ?

Q: The pH of a basic solution is 12.51. What is pOH?

A:

Q: What volume (in mL) of 15.8 M HNO, would be required to make 500.0 mL of a solution with a pH of…

A: Given:  15.8 M HNO3 500.0 mL of a solution with a pH of 3.20

Q: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

A:

Q: An aqueous solution at 25 C is 110% HNO, by mass and has a density of 1.046 g/mlL. What is the pH of…

A: Molarity of a solution is the number of moles of solute present in 1 liter of solution. The pH scale…

Q: Sodium hypochlorite solution, sold as “chlorine bleach,” ispotentially dangerous because of the…

A: NaClO is a salt of strong base NaOH and weak acid HClOThe anionic part ClO- undergoes anionic salt…

Q: What is pH of a solution consisting of 1.35 M NH3 and 2.08 M NH,NO,? K, of NH, is 5.8 x 10 10 0 9.13…

A: Given: Concentration of NH3 = 1.35 M Concentration of NH4NO3 = 2.08 M Ka for NH4+ = 5.8×10-10 We…

Q: Which one of the following 1.0 M solutions would have the highest pH?

A: A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value…

Q: A CHM 122 student combines 42.2 mL of 0.413 MHBR with 32.7 mL of 0.384 M KOH. What is the pH of the…

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Q: calculate the PH , of solution prepared by-14 addition of 85ml from NaOH ( 0.1M) to 75 * ? ml of HCI…

A:

Q: The pH of an aqueous solution at 25.0 °C is 12.36. What is the molarity of H + in this solution?

A: Given information,      The pH of an aqueous solution at 25.0 °C is 12.36

Q: Calculate the pH value for a 1:1 mixture of 0.003 M Ca(OH), (aq) and 0.002 M HCI (aq). Provide your…

A: Given : Concentration of Ca(OH)2 = 0.003 M Concentration of HCl = 0.002 M And the mixture is 1 : 1…

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.