# How is the pH of a strong acid compared to a weak acid of the same concentration?

14,682 results
1. ## science

Which acid-base chemical reaction is irreversible?(1 point) strong acid added to water water on its own weak base added to water weak acid added to water Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric

2. ## chemistry

Strong base is dissolved in 665 mL of 0.400 M weak acid (Ka = 3.69 × 10-5) to make a buffer with a pH of 3.94. Assume that the volume remains constant when the base is added. HA(aq) + OH-(aq) -> H2O(l) + A-(aq) Calculate the pKa value of the acid and

3. ## Chemistry

Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is added to the buffer

4. ## chemistry

Is this a buffer system? NH3/(NH4)2SO4? It is formed by mixing NH3 (weak base) and a strong acid (H2SO4), but according to my worksheet it is not a buffer system. Why is this so? Isnt it a buffer as long as it consists of a weak base and its salt of a

5. ## CHEMISTRY

HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong acid (HNO3);

6. ## chemistry

A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH

7. ## Chemistry

Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number

8. ## Chm 2

The question asks, Consider the following weak acids and their Ka values Acetic acid Ka = 1.8x10^-5 Phosphoric acid Ka = 7.5x10^-3 Hypochlorous acid Ka = 3.5x10^-8 What weak acid-conjugate base buffer system from the acids listed is the best chouce to

9. ## Chemistry

Why is the reaction rate of a given metal with a stronger acid is faster than with weaker acid? Which one required more volume to produce neutral solution, a strong acid or strong base,or are they just the same? Can you explain it to me please coz I can't

10. ## chemistry

Lactic acid is a weak acid with the formula , HCH3H5O3, the Ka for lactic acid is 1.38 x 10-4. In aqueous solution, lactic acid partially dissociates according to the following reaction: HCH3H5O3 ⇔ CH3H5O3- + H+ Use the Ka equation to calculate the pH of

11. ## Chemistry

Find the pH of mixture of acids. 0.185 M in HCHO2 and 0.225 M in HC2H3O2 Im using an ice chart of weak acid and putting in strong acid in H+ initiAL concentration. I've done the problems many different ways but cannot seem to get the right answer help

12. ## Chemistry

The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid. a. Write an equation for the above reaction. b. Calculate the molarity of the weak acid c. Write the equilibrium equation. Construct a table

13. ## Chemistry

1. As the strength of a weak acid increases, the proportion of ions to molescules increases or decreases? ... I think that it will increase. Is this right? 2. As the as the concentration of a weak acid increases, the pH... decreases? Is decreases correct?

14. ## chemistry

do we have buffering region and ph=pka in any of these conditions: strong base vs strong acid strong base vs weak acid weak base vs strong acid weak base vs weak acid

15. ## AP Chemistry

Rank these compounds in order of increasing hyroxide ion concentration: weak base, weak acid, strong base, strong acid.

16. ## Chemistry

A substance of Ka of 1 x 10^–5 would be classified as a ____. A.strong acid B.weak acid C.strong base D.weak base I think it is B...?

17. ## chemistry

Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?

18. ## Chemistry

If an equal number of moles of the weak acid HOCN and the strong base KOH are added to water, the resulting solution will be acidic, basic or neutral? There is a complicated answer and a sensible answer. Both arrive at the same answer. But here is the

19. ## Chemistry-Dr Bob help!!

0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of

20. ## Chemistry - Buffers

A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer? A. .01 mol B. .05 mol C. .10 mol D. .15 mol E. .20

21. ## Chemistry

Which of the following result in buffered solutions when equal volumes of the two solutions are mixed? a.) .1 M HCl and .1 M NH4Cl b) .1 M HCl and .1 M NH3 c.) .2 HCl and .1 M NH3 d.) .1 M HCl and .2 M NH3 By def. I know that a buffed solution is made from

22. ## chemistry

Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone

23. ## chemistry- check!

1. A pure salt solution can be any of the following except a. basic b. buffered *** c. alkaline c. acidic 2. You can make a buffer with all the following except a. weak acid + conjugate base b. weak base + salt of weak base c. strong acid + salt of strong

24. ## Chemistry

why is a weak acid weak base titration different from strong acid strong base/ weak acid strong base/strong acid weak base?

25. ## Chemistry

i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=2×10-3 or one with Ka=8×10-6 c. a 0.1 M solutions of

26. ## Acid-Base chem

Which of the following would for a buffer if added to 250.0 mL of .150 M SnF2? a).100 mol HCl b).060 mol HCl c).040 mol HCl d).040 mol NaOH e).040 mol HF I figured I could find out the pH of the solution with HCl/NaOH/HF added, and then find the pH when

27. ## chemistry

The pH of a certain acid having a concentration of 0.20 M was measured. The pH was 2.50. Was this a strong or a weak acid? I answered it is a strong acid because strong acids have a lower pH. I am just not too sure if there is anything missing in my

28. ## chemistry (buffers)

How can weak acid nitrous acid HNO2 form a buffer solution with equal concentrations and volumes with weak base NH3? I thought that buffer solutions only occured between weak acids and strong bases or vice versa. The example above as two weak soltuions.

29. ## chemistry

#1)hydrochloric acid is a relatively strong acid . imagine that HCl is added to a buffer solution containing the weak acid phosphoric acid and a salt a)will HCl react with weak acid (H3PO4), or will it react with the salt (Na2HPO4)? b)one product of this

30. ## Chemistry

A buffer is prepared by mixing 110. mL of 0.442 M HCl and 0.545 L of 0.400 M sodium acetate. How many grams of KOH must be added to 0.500 L of the buffer to change the pH by 0.10 units? The pH I have calculated to be 5.28. What do I to figure this out? I

31. ## chemistry 12

The pH of a certain acid having a concentration of 0.20M was measured. The pH was 2.50. Was this a strong acid or weak acid?

32. ## Chemistry

What are the general equations for reaction of 1. Strong acid and weak base 2. Strong base and weak acid?

33. ## Chemistry

Part A: Unknown Acid use 1gram and mix with 120 mL of distilled water Determine the concentration of the acid by titrating with 0.0998 M of NaOH Concentration of NaOH= 0.0998M Volume of NaOH= 3.5 mL # moles of NaOH= Initial Concentration of Weak Acid- Show

34. ## chem

Can someone please help me by explaining and correcting me? 1) A 0.057M solution of a weak acid has a pH of 4.93. Determine the ionization constant, Ka, of the acid. a) 2.1 x 10^-4 b) 2.4 x 10^-9 c) 4.1 x 10^-8 d) 2.8 x 10^-7 e) 1.4 x 10^-10 -- To be

35. ## Chemistry

Salt of a Strong Base and a Weak Acid. pH of Solution. Calculate the pH of a 5.90×10-1 M aqueous solution of sodium nitrite (NaNO2). (For nitrous acid, HNO2, Ka = 4.00×10-4).

36. ## Chemistry

Ammonia (NH3) is a weak base with a Kb= 1.8 X 10^-5 and hydrochloric acid (HCl) is a strong acid. What is the pH of a mixture made by adding 6.61 grams of NH4Cl to a 412 ml of a 0.180M solution of NH3?

37. ## Chem+ASAP+2 fill in the blank questions+ASAP!!!

PLease check this. They are fill in the blank and I just need to know if they are right. Thanks! 9. Compared to a strong acid-strong base titration curve, a weak acid-strong base titration curve has a (higher, lower) __higher___ initial pH value. 10.

38. ## Chemistry

Determine if the ffg are strong, weak, nonelectrolytes: Sulfuric acid - strong? Potassium hydroxide - strong? Carbonic acid - strong? Propyl amine - weak? Potassium iodide -weak? Ethanol - strong ? Glucose - nonelectrolyte? am i right?

39. ## Chemistry

Classify the following as: Weak or strong acid, weak or strong base, salt (from weak/strong acid and base). If appropriate, split the formula into its component ions. HNO3 So far, all I have is: HNO3 + H2O -> NO3^- + H3O^+ And I know HNO3 is a strong acid.

40. ## chem

What is the difference between a weak acid and a dilute acid: a strong acid and a concentrated acid? Give an example of each

41. ## acids,bases and salts

1.What is meant by a weak and strong base?Give two formulae of strong bases. 2.state the name of the base that is considered to be weak. 3.Amphoteric oxide?give two examples. 4.Alkali?two examples. 5.Neutral oxides;two example. 6.Acid anhydride. (ii)write

42. ## chemistry

hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M

43. ## Honors Chemistry

I need someone to check these questions. I know its a lot of questions. 2NH3 + Ag+ Ag(NH3)2+ a. What is the Lewis acid in this equation? [Ag+] b. What is the Lewis base in this equation? [NH3] Given H2SO4 is sulfuric acid, HNO3 is nitric acid, and H3PO4 is

44. ## chemisty

0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid (NaX) to 100.0 mL of

45. ## CHEMISTRY

How can we determine the equivalence point ( or end point ) in the curves in titration ( strong acid/weak base and weak acid/strong base )

46. ## chemistry

hello, I can't seem to solve this question. i tried to look up someone else who may have asked this question. I found this girl named Sara,but her answer didn't really help me much because it did not answer the question. What is the pH when enough 0.10 M

47. ## Chemistry

me again 8. You are given two beakers, A and B, with colorless liquids in htem. What two tests would you perform to determine which one is a strong acid and which one is a weak acid? Be specific with the test and the results as well as how you would

48. ## m.e.i.pampore

if we tritrate weak acid(oxalic acid)with strong base(naoh).which indicator is used and why

49. ## chemistry

Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?

50. ## Chemistry

I have a compound (mx) weak acid (x- = Hx) mx in 5M strong acid solution solubility = 5x10(-3) Ksp = 1x10(-20) Find Ka... I need to know where to start

51. ## Chemistry (A level)

I was given a Chemistry question on the titration of a strong base being added to a weak acid. The question was: "Calculate the pH in a titration when 10.0cm^3 of a 0.10moldm^-3 solution of NaOH is added to a 10.0cm^3 of 0.25moldm^-3 solution of ethanioc

52. ## Chem

What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH C6H5COOH

53. ## Chemistry

When will a salt produce a neutral solution? 1-if it contains the conjugate base of a strong acid 2-if it contains the conjugate base of a weak acid 3-if it contains the conjugate acid of a weak base

54. ## Chemistry

The pH of an 0.0870 M solution of weak acid A is 2.20. The pH of an 0.0830 M solution of weak acid B is 4.07. The pH of an 0.0890 M solution of weak acid C is 5.13. Identify the three acids from among those listed below (the Ka values are listed in

55. ## chemistry

2- A 0.310 M solution of a weak acid, HX, has a pH of 2.53 a. Find the [H+] and the percent ionization of nitrous acid in this solution. b. Write the equilibrium expression and calculate the value of Ka for the weak acid. c. Calculate the pH of the

56. ## Chemistry

A 0.108 M sample of a weak acid is 4.16% ionized in solution. what is the hydroxide concentration of this solution? I know that i set up an ice table. The equation would be weak acid + H20 goes to OH + the acid. What do i do with the 4.16 %? How does that

Sulfuric acid is a diprotic acid, strong in the first ionization step and weak in the second (Ka2=1.1X10^-2). Using appropriate calculations, determine whether it is feasible to titrate 10.00mL of 0.1 M H2SO4 to two distinct equivalence points with 0.1 M

58. ## AP Chemistry

A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak

59. ## AP Chemistry

A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or a weak acid with a weak

60. ## Chemistry (Titration Curves)

Which of the following Acid+Base titration combinations would have a buffering region in their plot? 1)Strong Acid+Strong base (HCl+NaOH) 2)Weak acid and strong base (Acetic+NaOH) 3)Strong Acid and weak base (HCl+NH3) 4)Weak Acid and weak base (Acetic+NH3)

61. ## Chemistry

An unknown monoprotic acid has a pH of 2.87. Is this acid weak or strong if 22.32 mL of 0.112 M NaOH is required to titrate 25.00 mL of the acid? If the acid is weak, calculate its Ka. Answer is Ka = 1.8 x 10^-5, but I don't know how to get there. Any help

62. ## chemistry

Can you tell if I'm correct. Which combination in titration has ph=pka and buffer region strong acid-strong base- no to both strong acid-weak base- yes to both weak acid-strong base- yes to both weak acid-weak base- I'm not sure about this one. Can anyone

63. ## Science

How is the pH of a strong acid compared to a weak acid of the same concentration?

64. ## Chemistry

You have two buffer solutions 1) weak acid and its conjugate base 2)weak base and its conjugate acid. Write explicitly ( considering generic formula for acid and base) the equations of neutralization when you: a) add strong acid and strong base 1) b) add

65. ## chemistry

if 0.4M NaOH is titrated with 0.4M HF, how do we calcualte the ph at equivalence. The book assumes each is 1L, but why do we use 1L * chemistry - Dr.Jim, Thursday, November 11, 2010 at 5:31am HF is a weak acid, so you need the dissociation constant. The pH

66. ## Chemistry

In the titration of a weak acid with a strong base, the pH at the equivalence point is affected mostly by a.hydrolysis (reaction with water) of the weak acid b.the dissociation of water molecules c.the presence of excess base d.the hydrolysis of the

67. ## chemistry

A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following statements best explains

68. ## Chemistry

When diluting a weak acid and a strong acid, why is it that the pH changes more significantly in the strong acid? (consider the equilibrium occurring) With HCl

69. ## Chemistry (Ionic Equilibria)

When a WEAK acid can be said to be weak, and when a WEAK acid can be said to be strong? I only know the difference between weak acids and strong acids, but i don't know that even weak acids can be classified as weak and strong. Plz help

70. ## chem

What is the difference between a weak acid and a dilute acid: a strong acid and a concentrated acid? Give an example of each

71. ## SCIENCE PLZZ HELP!!!

Given equal concentrations, which of the following produces the fewest hydronium ions in an aqueous solution? strong acid weak acid strong base weak base This is the only question i need help on and i have no clue what ut is! any help?

72. ## Chemistry

I don't understand how to work out the volumes of weak acid and strong base to mix to make 1L of buffer when given the concentrations of weak acid and strong base (in my case 0.160M NaOH and 0.200M H3PO4) and the pH required (7.00). Specifically the

73. ## Chemistry

I don't understand how to work out the volumes of weak acid and strong base to mix to make 1L of buffer when given the concentrations of weak acid and strong base (in my case 0.160M NaOH and 0.200M H3PO4) and the pH required (7.00). Specifically the

74. ## Biochemistry

You are told that the solutions in two beakers are both 0.02 M solutions of acids "A" is weak acid and acid "B" is a strong acid. Which of the two acids would have the lower pH, acid "A" or acid "B"? Explain your answer.

How would an HA acid behave in water if it were a strong acid, weak acid, and non-electrolyte?

76. ## CHEMISTRY

Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number

77. ## chemistry

Choices: True,False. Select all that are True. The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because of the presentce of the conjugated acid in the water. One cannot prepare a buffer from a strong acid and

78. ## chem

Acetic acid is a weak acid with the formula , CH3COOH, the Ka for acetic acid is 1.76 x 10-5. In aqueous solution, acetic acid partially dissociates according to the following reaction: CH3COOH ⇔ CH3COO- + H+ Use the Ka equation to calculate the pH of

79. ## Chemistry

TRUE OR FALSE? 1) A solution that is made out of 1.00mol/L ammonia and 0.50mol/L of ammonium chloride is a basic buffer. 2) The pH at the equivalence point of a weak base with a strong acid is expected to be less than 7 because the acid that is added is

80. ## Chemistry

1 g of acid was mixed with 120 ml of distilled water and the solution was filtered into a clean dry beaker. A 25 ml aliquot of this solution was titrated with 0.1120 M NaOH. The pH of the acid was recorded to be 4.42. Calculate the initial concentration of

81. ## CHEMISTRY RIDDLE!!!!

hi! i was just wondering if you could help me figure out this riddle!! im absolutely stumped!!! "Anger: an acid that can do more harm to the vessel in which it is stored, than to anything on which it is poured" is a quote attributed to Seneca, a Roman

82. ## CHEMISTRY

Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid and determine the number

83. ## chemistry

At what point in the concentration of the weak acid or conjugate base does the buffer solution stop resisting a PH change when strong acid is added ? Thank for helping

84. ## Chem. Again

28: You have a glass of pure water. Are chemical reactions occurring in the water? If so, what are they? If not, explain why not. 29: While investigating the effects of acid rain in your area, you discover a lake that is surprisingly resistant to changes

85. ## Chemistry

What is the pH of the solution created by combining 2.50 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? I believe if my calculations are correct the answer is 1.28 however i do not know how to answer this question because it has a weak acid

86. ## titrations

I have to find the correct acid-base indicator to use for the following titrations (methyl orange with end point @ pH 4, bromthymol blue with end point @ pH 7, or phenopthanlein with end point @ pH 9). I have several problems given to me, but first I'm

87. ## Chemistry

i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=2×10-3 or one with Ka=8×10-6 c. a 0.1 M solutions of

88. ## chemistry

I am giving a titration curve of a weak base and strong acid. The pH on the y scale is from 0-14 and the volume of titrant in mL is from 0-34. It looks like the equivalene point is around 22? The question is: "The above titration curve was obtained when a

89. ## Chemistry

I took 25 mL of an unknown weak acid and added it to 10 mL of NaOH solution. I measured the pH and got 2.88 with concentration of NaOH @ .0098 and weak acid at 0.0102. What is pKa for the acid?

90. ## CHEMISTRY

What indicator is better in the following titrations : 1) strong acid/strong base a) methyl red (4.4 - 6.2 ) b) bromophenol blue (6.2 - 7.6 ) 2) strong acid/weak base a) methyl orange (3.1 - 4.4 ) b) bromophenol blue (3.0 - 4.6 ) 3) weak acid/strong a)

91. ## Chemistry

Is an ammonium an acid or s base? Is it strong or weak? Is it a weak, acid?

92. ## Chemistry

Is it possible to make a buffer with a strong acid and a strong base? So I know a buffer consists of a weak acid and its conjugate base or a weak base and its conjugate acid. And I believe it is possible to make a buffer with a strong acid and weak base or

93. ## Chemistry

Is it possible to make a buffer with a strong acid and a strong base? So I know a buffer consists of a weak acid and its conjugate base or a weak base and its conjugate acid. And I believe it is possible to make a buffer with a strong acid and weak base or

94. ## Chem!

does the addition of a strong acid increase the percent ionization of a weak acid HB?

95. ## Chemistry

A monoprotic acid of 0.065 M concentration has a pH of 2. 75. Is this a strong or weak acid?

96. ## chemistry

I need help setting up a problem to calculate pH during the titration of 20.00ml Of 0.1000M (CH3CH2)3N (Kb= 5.2 x 10-4) with 10.00ml of .1000M HCL. I can do it with a weak acid - strong base but this is a weak base - strong acid and I don't know if its the

97. ## Chemistry

Consider 2 separate solutions, one of a weak acid HA and one of HCL. Assume that you started with 10 molecules of each. Draw a picture of what each solution looks like at equilibrium. Ok to my very limited knowledge on this subject so far, a weak acid at

98. ## Chemistry

i. Which of the following solutions has the lowest pH (more acidic). Explain you answers. a. a 0.1 M solution of a strong acid or a 0.1 M solution of a weak acid. b. a 0.1 M solution of an acid with Ka=2×10-3 or one with Ka=8×10-6 c. a 0.1 M solutions of

99. ## Chemistry

How do you find the initial concentration of the acid give the titration curve of a weak acid-strong base titration?

100. ## Chemistry

Hello, I'm wondering what the difference is in method when it comes to finding the pH of a weak acid versus finding the pH of a strong acid? Thanks!