16. Calculate the K, for an unknown acid HX, given that a 0.25 M salt solution NaX has a pH of a 8.48.

Q: would

A: [H+] = mass of HCl / [ molar mass of HCl • volume of HCl Solution ]  [H+] = 0.500g / ( 36.46gmol-1 •…

Q: How many moles of H3O+ or OH- must you add to 87.5 mL of HA solution to adjust its pH from 8.92 to…

A: Initial pH = 8.92 Therefore [H+] = 10^(-pH) = 10^(8.92) = 0.012 * 10^ -7 Final pH = 6.33Therefore…

Q: 69. A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant…

A: A weak acid are those which does not completely dissociate to liberate H+ ion

Q: The K, of yittrium hydroxide, Y(OH),(s), is 1 x 10 22 at 298 K. The pH of this solution to one…

A: The product of equilibrium concentrations of the constituent ions raised to the power equal to their…

Q: Calculate pH for a solution that contains proton [H+] of 0.02 mM (milimole/L).

A: Given: The concentration of proton [H+] is 0.02 mM

Q: Calculate [H3O+] for each solution pH = 1.52?

A: pH = -log [H3O+]

Q: Consider the reaction below. Which species is(are) the Brønsted-Lowry acid(s)? HF (aq) + NH3 (aq) =…

A:

Q: If the K, of a weak base is 7.2 × 10-6, what is the pH of a 0.33 M solution of this base? pH =

A: in this question given data is  α=KaC   ka×kb=10-14C=0.33MPH=-logH+ Apply the value given formula,…

Q: A certain weak base has a ?b of .8.40×10−7. What concentration of this base will produce a pH of…

A: Assuming the weak base is monoprotic which can be written as BOH. Hence the dissociation reaction of…

Q: A solution is prepared by adding NaOH to pure water until a pH = 9.34 is obtained. Calculate the pH…

A:

Q: Consider a HCl solution that has a pH of 4.70. a) Calculate the concentration of HCl.  b) Identify…

A:

Q: Pyridine, CSHSN, behaves as a base in aqueous solution. A solution of pyridine with an initial…

A: Given that: pH = 9.562 molarity of pyridine = 0.750 M To find: Kb for the compound?

Q: Calculate the pH of a 0.0010 M solution of HB, a hypothetical acid with K = 9.6 x 10$. (Use th…

A: The pH of 0.0010 M HB solution is calculated as shown below.

Q: When calculating the [H3O+} for a polyprotic acid, the second ionization step can often be…

A: Polyprotic acids are capable of releasing more than 3 protons. The ionization constant value for the…

Q: PRE A Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…

A:

Q: If the ?b of a weak base is 5.0×10−6, what is the pH of a 0.28 M solution of this base?   pH=

A: pH + pOH = 14

Q: In calculating [H;Oʻ] for a mixture of a strong acid and weak acid, the weak acid can often be…

A: The acid is the one that can donate the proton or accepts the pair of electrons.  According to…

Q: How many moles of nitric acid do you have in a 0.650 L solution of 0.035 M nitric acid? What is the…

A: a) Calculate the moles of nitric acid in a 0.650 L of 0.035 M nitric acid. Given: Volume of nitric…

Q: If the ?b of a weak base is 5.9×10−6,5.9×10−6, what is the pH of a 0.28 M 0.28 M solution of this…

A:

Q: Please help me, double check your answers as previous tutors got it wrong.

A: pH is the potential of the hydrogen or the power of the hydrogen. It basically explains how acidic…

Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: Calculate the [H3O+] and pH of each H2SO4 solution. At approximatelywhat concentration does the x is…

A: Given:-                To Calculate the [H3O+] and pH of each H2SO4 solution. At approximately what…

Q: A 0.27M Solution of this week acid has a pH of 2.59 determine the Ka Of the weak acid

A:

Q: 2. For each of the following salts, determine the pH of a 2.50M solution of the salt. You will need…

A: Molar concentration of solution of salt = 2.50 M

Q: The K₂ of HClO₂ is 0.010. Determine the pH of a 0.1 M HClO₂ aqueous solution at equilibrium.

A:

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.80. What is the Kb of this…

A: Welcome to bartleby!  Introduction :  We have to calculate Kb of the base .

Q: rder these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine…

A: The question is based on the concept of acidity. we have to arrange the given molecules according to…

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

A:

Q: For a solution of 0.15 M HF, the [H+]  0.15 M.  Why?  What is the [H+]?  What is the pH of the…

A:

Q: Find PH of solution 0.023M solution of HCI?

A:

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: Calculate [H+] for each of the following solutions, andindicate whether the solution is acidic,…

A: pH = -log[H+] pOH = -log [OH-] pH + pOH = 14

Q: 30.0 mL of 0.1M KOH is diluted with water until the final volume is 300 mL. CALCULATE: pH  of the…

A: Molarity is defined as the ratio of number of moles of the substance to the volume of the solution…

Q: A 0.350M solution of acetic acid has a pH of 2.60 @ 25°C. Determine the Ka of acetic acid.

A: Given, Concentration of acetic acid = 0.350M. pH of acetic acid = 2.60. The concentration of H+ can…

Q: What is the pH of a 6.20 x 10-3 M NaOH solution?  (This solution is basic, concentration is of OH-)

A:

Q: A certain benzoic acid solution has pH = 2.54. Calculate the volume of 0.0979 M KOH required to…

A: The neutralization reaction is the type of the reaction in which an acid is treated with a base to…

Q: Calculate the pH and pOH of an aqueous solution that is 0.75 % HCI, by mass, and has a density of…

A: Given :-  % by mass of HCl = 0.75%  density of solution = 1.04 g/mL  To calculate :-  pH and pOH for…

Q: A certain weak base has a ?b of 8.40×10−7. What concentration of this base will produce a pH of…

A: Weak base dissociated less in solution

Q: As much as 8 grams of NaOH (Mr = 40) is dissolved in water until the volume of the solution becomes…

A:

Q: a key component of understanding weak acids isntheir Ka values which are just equillibrium…

A:

Q: A 1.57 M solution of a weak acid HA is found to have a pH of 2.05.     Determine the pH of a 2.00 M…

A: The concentration of hydrogen ions can be calculated as follows-

Q: Express the pH of the solution ot three decimal places. 20.00 mL of 1.20 M HCl diluted to 0.570 L

A: Initial concentration, M1 = 1.20 M Initial volume, V1 = 20.00 mL Final volume, V2 = 0.570 L = 570 mL

Q: significant When determining the pH of a polyprotic acid solution or mixture of acids, only the [OH…

A: We know that, polyprotic acids are that kind of acids, which have more than one deionized hydrogen.

Q: Calculate the pH of a 0.300 M NaF solution. The K, value for HF is 7.20 x 10-4. Will the solution be…

A: NaF is salt and made of strong base Sodium hydroxide (NaOH), and a weak acid, Hydrofluoric acid…

Q: In the laboratory a student measures the percent ionization of a 0.558 M solution of formic acid ,…

A: The dissociation of formic acid: Concentration of formic acid =0.558M. Percentage ionization of…

Q: A certain weak base has a K, of 8.20 x 107. What concentration of this basc will produce a pH of…

A: Given, pH= 10.29 Kb = 8.20*10-7

Q: A 0.025 M solution of a weak acid (HA) has a pH of 4.28. What is the K, of the acid? a

A: ka is the ratio of  product of concentration of products raised to their stoichiometric coefficient…

Q: According to Lewis acid-base theory, a base is defined as alan OA electron acceptor O B. proton…

A: Lewis base : Lewis base is a substance which have tendency to donate lone pair of electron (non…

Q: solution is 3.75. what is the percent ionization for

A: Concentration of Acid(C) = 0.012 M pH = 3.75 pH = -log([H+)] = 3.75 [H+] = 10-3.75 = 0.000178 M

Q: A certain weak base has a K, of 8.80 x 10-7M. What concentration of this base will produce a pH of…

A: Given data: The Kb value of weak base = 8.80×10-7. The pH of the weak base = 10.28. To calculate:…

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.