What is the pH of 100 mL of a solution made using 5 mL of 1 M Na2 HPO4 and 5 mL of 1 M NaH2PO4?

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: Calculate the [OH-] and pH of a mixture formed by adding 50.0 mL of 0.0.20 M HCl to 150 mL of 0.010…

A: Given : Concentration of HCl = 0.020 M                                                     (Assuming…

Q: You are given an HI solution at pH 1.3. How much water do you need to add 0.050 L of this solution…

A: ⊙we know,   PH=-log[H+]⇒[H+]=10-PH⊙concentration=no.of molesvolume⊙No. of moles= concentartion *…

Q: What is the pH of a solution that is 0.10 M in HCIO (K₂= 3.5 × 10-8) and 0.10 M in HCI? a

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Q: What volume (mL) of 0.1M NaOH will be needed to titrate 20.00 mL of 0.1M HNO3?

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Q: Calculate the pH of the resulting solution when 100.0 mL of 0.2 M HNO2 is titrated by 0.1 M NaOH…

A: when 200.0 mL of NaOH is added Given: molarity, M(HNO2) = 0.2 M volume of, V(HNO2) = 100 mL M(NaOH)…

Q: A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 ×…

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Q: What is the pH for a 400 ml solution of 1.6 M Benzoic Acid if you added 175 grams of conjugate base…

A: The solution is given below -

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of…

A: Given data contains, Volume of acetic acid is 45.00mL. Molarity of acetic acid is 0.10 M. Volume of…

Q: What is the pH of a solution of 100 mL of 0.025 M HBr and 100 mL of 0.10 M NaF? (HF Ka= 7.2 x 10-4)

A: Given Volume of HBr solution = 100 mLConcentration of HBr solution = 0.025 MVolume of NaF solution =…

Q: What is the pH of a solution obtained by mixing 100ml of a 0.01M NaOH solution and 100ml of a 0.01 M…

A: NaOH is a strong base and Acetuc acid is a weak acid, thus we will get a overall solution basic.

Q: What

A: Dear student I have given answer to your question in the image format.

Q: How can we answer this question: 1) Equal volumes of 1 M solutions of citric acid, sodium citrate,…

A: A weak acid shows that doesn't ionize promptly in an aqueous solution. The weak acids contain low…

Q: Predict whether the following aqueous solutions have a pH less than 7, very close to or equal to 7…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: Calculate the pH of a solution that contains 3.25 M HCN (K a = 6.2 x 10 -10 ), 1.00 M NaOH and 1.50…

A: Detail

Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

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: In the titration of 70.0 mL of 0.400 M HCOOH with 0.150 M LIOH, how many mL of LiOH are required to…

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Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

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Q: The first equivalence point for 40.00 mL of 0.1000M H3PO4 is reached when 21.38 mL of 0.1871 M NAOH…

A: The pH of the solution is the power of protons in the solution. While pOH is related to the basicity…

Q: What is the pH of a solution containing a mixture of 0.050 M HC2H3O2 and 0.025 M NaC2H3O2?  (Ka =…

A: Given: [HC2H3O2]=0.050 M [NaC2H3O2]=0.025 M Ka = 1.8 × 10-5 pKa=-log (1.8 × 10-5) pKa=4.745

Q: How many grams of lactic acid and mL of 0.1M sodium hydroxide must be added to 100 mL of water to…

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Q: What is the pH change when 40.0 mL of 0.100 M NaOH solution is added to 40 mL of 0.100 M H3PO4…

A: Volume of 0.1 M NaOH solution = 40 mLVolume of 0.1 M H3PO4 solution = 40 mL

Q: How many grams of KOH would you have to add to a 2.1 M/450 ml sample of HCl to make the final pH 11?

A: Balanced Reaction HCl + NaOH --> NaCl + H2O HCl reacts with NaOH to produce water and NaCl

Q: Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given Molarity of KOH = 0.150 M Volume of KOH = 10 ml Molarity of HBrO = 0.300 M Volume of HBrO = 20…

Q: What is the pH when 20.0 mL of 1.00 M NaOH has been added to 25.0 mL of 1.00 M CH3COOH…

A: Calculation of no. of mmol of NaOH: n=Molarity×Volume=1.00 M×20.0 mL=20 mmol Calculation of no. of…

Q: What is the pH of a solution prepared by mixing 15.0 mL of 0.24 M KOH and 25.0 mL of 0.24 M of…

A: Given data : Concentration of KOH = 0.24 M Volume of KOH = 15.0 mL Concentration of HClO = 0.24 M…

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.