What is the pH of a solution containing 0.12 mol/L of NH4Cl and 0.03 mol/L of NaOH (pKa of pKa NH4+/NH3of is 9.25)?

Q: What volume of 0.120 M NaOH must be added to 100 mL of 0.100 M NaHC204 to reach a pH of 4.70? H2C204…

A: The solution is given below -

Q: A 0.045 0 M solution of HA has a pH of 2.78. Find pKa for HA.

A: Given, initial concentration of HA = 0.0450 M             pH = 2.78 We know that, pH can be…

Q: A known organic acid has pKa= 3.80. What is the percent dissociation of this organic acid in a…

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Q: a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to…

A: Thankyou for posting your question but I am doing only (a) subpart because it seems that (b) and (c)…

Q: A 11 mM solution of a compound with a pKa = 6.5(1L total) has a pH of 7.5.If a biochemist adds 9…

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Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Ka = 4.5*10^-4 (given) pKa = – log [ Ka ] = – log(4.5*10^-4) = 3.347 Now, By using Henderson…

Q: that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Kaof lactic acid is 1.4 × 10-4.…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: What is the pH of a solution that is 0.01M in picric acid and 0.1M in sodium picrate. (pKa=0.38)

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Q: If 90.00 mL of a 1.780 MHNO2 solution is reacted with 1.950g NaOH, calculate the resulting pH. The…

A: Given : Volume of HNO2 = 90 ml  Molarity of HNO2 = 1.780 M

Q: A solution made with 0.140 moles of phosporic acid (H3PO4), dissolved in 194 mL of solution, was…

A: Moles of H3PO4 = 0.14 Volume of solution of H3PO4 = 194ml = V2 Concentration of NaOH = M1 = 1.320M…

Q: If the pKa of HCHO 2 is 5.74 and the pH of an HCHO 2/NaCHO 2 solution is 6.11, which of the…

A: A buffer solution is a that type of solution in which if we add a small amount of acid or base then…

Q: A solution containing 0.200 M for ion X- and 0.180 M  HX has a pH of 9.22. What is the pKa of HX?

A: Since the solution is having X- i.e conjugate base of HX and acid HX. Hence the solution is a buffer…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.250 M CH₃NH₃I? (Kb of CH₃NH₂ is

A: The question is based on the concept of PH calculations. we have to apply henderson equation to…

Q: 1. A 0.0722 M solution of a weak acid has a pH of 3.11. Calculate the Ka of this acid.. х 10-6 2. A…

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Q: The pka of HCN = 9.31. Which solution, when added to 10.0 mL of 0.10 M HCN, has a pH of 9.31? O 10.0…

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Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC₂H₃O₂] + [C₂H₃O₂⁻] = 0.250 M) at pH…

A: Volume of acetate buffer = 0.5 L. Concentration of acetate buffer = 0.250 M Moles of acetate buffer…

Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC2H;O2] + [C2H3O2] = 0.250 M) at pH…

A: pH is used to determine the concentration of hydronium ion.

Q: Describe how to prepare 0.500 L of 0.100 M imidazole buffer, pH=7.50, pKa= 6.99 starting with…

A: Henderson-Hasselbach equation shows the relationship between pH of a solution, the acid dissociation…

Q: Calculate the pH of a buffer solution containing 0.25 M NH3 and 0.34 M NH4NO3. Data: pKa (NH4+) =…

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Q: You wish to prepare an HC2 H3 O2 buffer with a pH of 4.14. If the pKa of HC2H3 O2 is 4.74, what…

A: Given :-   pH of buffer solution = 4.14  pKa value for HC2H3O2 = 4.74  To calculate :-  Ratio of…

Q: The pKp of 4-hydroxypyridine is 10.80 at 25°C. What is the pH of a 0.0250M solution? Round to two…

A: Please have a look on the solution below:

Q: What is the pH of a solution of 12.01 g NaHSO4 (120.07g/mol) and 17.05 g Na2SO4 (142.05g/mol)…

A: The pH of a solution of 12.01 g NaHSO4 (120.07g/mol) and 17.05 g Na2SO4 (142.05g/mol) dissolved in…

Q: What is the pH of a solution

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Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC₂H₃O₂] + [C₂H₃O₂⁻] = 0.250 M) at pH…

A: How many mL of 1.000 M NaOH must be added in order to change the pH of acetate buffer to 5.23 from…

Q: what is the Ka value

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Q: What is the pH of a solution that has 0.125 M CH3COOH and 0.125 M H3BO3? Ka of CH3COOH = 1.8 × 10−5…

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Q: What is the pH of a solution containing 0.30 M CH₃COONa and 0.10 M CH₃COOH? The Ka of CH₃COOH is 1.8…

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Q: 1. Calculate the pH of a 1 L solution containing 6 mL of 1.5 M acetic acid and 5 ml of 0.4 M sodium…

A: According to Henderson- hasselbalch equatlon.pH=pKa+log[salt ][acid]..........1stGiven,pKa=4.766ml…

Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC₂H₃O₂] + [C₂H₃O₂⁻] = 0.250 M) at pH…

A: pH is used to determine the concentration of hydronium.

Q: A salt (MA) is dissolved in water. Given the values of ka and kb below, would the salt be considered…

A: If kb is greater than ka then solution is basic . And if ka is greater than kb then solution is…

Q: What masses of dimethylamine and dimethylammonium chloride do you need to prepare 5.00 Lof pH-12.00…

A: Given : pH of buffer = 12.00  Volume of solution = 5.00 L And total concentration of base and its…

Q: A solution made with 0.130 moles of phosporic acid (H3PO4), dissolved in 183 mL of solution, was…

A: Given: Concentration of NaOH = 1.160 M. Moles of H3PO4 = 0.130 mol. Volume of H3PO4 solution = 183…

Q: What is pOH of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3? Ka of NH4 + is 5.8 x 10-10…

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Q: You have 0.600 L of an 0.300 M acetate buffer solution (i.e. [HC2H3O2] + [C2H3O2] = 0.300 M) at pH…

A: We are provided with 0.600 L of 0.300 M acetate buffer solution having a pH of 5.30. We are required…

Q: mandalorious acid is a weak acid that reacts with water: HMaO2 (aq) + H2O (l) MaO2- (aq)+ H3O+…

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Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC2H;O2] + [C2H3O2¯] = 0.250 M) at pH…

A: Given data is: pH of buffer = 3.5 Let Concentration of [HC2H3O2]  be x M and concentration of…

Q: You have 0.500 L of an 0.250 M acetate buffer solution (i.e. [HC2H3O2] + [C2H3O2] = 0.250 M) at pH…

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Q: You have a solution of 100 mM sodium acetate (pH 4.50). The pka of acetic acid is 4.76. What is the…

A: Given: [CH3COONa] = 100 mM [CH3COOH] = x pH = 4.50 pKa = 4.76

Q: Calculate the pH of 3.5M citric acid solution at 25°C when the Ka is 7.1 x 104 (You'll need a RICE…

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Q: The pKa of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have…

A: Lactic acid and potassium lactate makes an acid buffer. Henderson equation is used to determine the…

Q: 5. A buffer solution contains 10.0 mmol of formic acid (HCOOH) and 15.0 mmol of formate (HCO0). If…

A: Given:Moles of Formic acid = 10.0 mmol.Moles of Formate ion = 15.0 mmol.PH of the solution =…

Q: a) Calculate how much water in mL must be added to dilute 75.0 mL 0.010 M HNO3 to a solution with pH…

A: Given,  75.0mL of 0.010 M of HNO3 diluted to a solution with pH = 3.0 the water added to a solution…

Q: How many moles of sodium acetate must be added to 500 mL of 0.25 M acetic acid solution to produce a…

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Q: What mass of Ca(OH) is required to neutralize 50.00 mL of 0.180 M HCI?

A: Given information:Volume of HCl = 50.00 mLConcentration of HCl = 0.180 M

Q: Creating a buffer system:    Desired pH = 6.4 What is the best acid to use? What is the pKa of…

A: According to Hendersen equation  pH = pKa + log [salt/acid] best acid can be carbonic acid  its pKa…

Q: A. What is the Kb when the Ka of a solution is 5.47x10^-4? B. the Ka of an acid is determined to be…

A: Hello. There are multiple questions posted together. The first question has been solved. To receive…

Q: Calculate the pH of 0.65 M of a weak acid HA with Ka = 2.56 x 10 -6.      5.59     2.89…

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Q: = 4.00 and pK, = 8.00. 10-23. The diprotic acid H,A has pK| (a) At what pH is [H2A] = [HA¯]? (b) At…

A: In this question, we have to find out the correct answer of given problem by the help of 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.